{"id":890,"date":"2025-06-27T19:05:28","date_gmt":"2025-06-27T19:05:28","guid":{"rendered":"https:\/\/blog.ajsrp.com\/en\/?p=890"},"modified":"2025-05-23T13:44:40","modified_gmt":"2025-05-23T13:44:40","slug":"how-to-calculate-percent-recovery-and-percent-yield-in-chemistry","status":"publish","type":"post","link":"https:\/\/blog.ajsrp.com\/en\/how-to-calculate-percent-recovery-and-percent-yield-in-chemistry\/","title":{"rendered":"How to Calculate Percent Recovery and Percent Yield in Chemistry"},"content":{"rendered":"

In chemistry, knowing how well a process works is key. Percent Recovery<\/strong> is a major way to check if a process is effective, mainly in making things pure and creating new substances.<\/p>\n

Figuring out the recovery rate<\/em> lets chemists see how much of a reaction they got. It also shows where they can make things better. By knowing how efficient a process is, scientists can make their methods better.<\/p>\n

Being able to figure out percent recovery<\/b> and yield is very important in chemistry. It’s used in lab work and big-scale production. This article will show you how to do these calculations and understand what they mean.<\/p>\n

Understanding the Basics of Chemical Calculations<\/h2>\n

Quantitative analysis is key in chemistry. It helps measure the success of chemical reactions. This lets chemists check how well their experiments work.<\/p>\n

The Importance of Quantitative Analysis in Chemistry<\/h3>\n

Quantitative analysis is the base for understanding chemical reactions. It lets chemists measure reactants and products. This way, they can see how much product they get and how to make it better.<\/p>\n

Key Metrics for Evaluating Chemical Reactions<\/h3>\n

When checking chemical reactions, several important metrics are used. These include how efficient the reaction is and how accurate and precise the results are.<\/p>\n

Efficiency Measurements<\/h4>\n

Efficiency metrics, like percent yield, show how much product is made. This is key for yield optimization<\/strong>. It helps find ways to improve the reaction.<\/p>\n

Accuracy and Precision Considerations<\/h4>\n

Accuracy and precision are also important. Accuracy is how close a measurement is to the real value. Precision is how consistent the measurements are. Both are needed for reliable recovery percentage<\/strong> calculations.<\/p>\n

What is Percent Recovery in Chemistry?<\/h2>\n

Percent recovery<\/b> is key in chemistry. It shows how much of a substance is found after a process. It helps measure how well a chemical process works.<\/p>\n

Definition and Fundamental Concepts<\/h3>\n

Percent recovery<\/b> is the ratio of what’s actually found to what should be found. It’s shown as a percentage. This is important for checking how well chemical processes work, like making new substances.<\/p>\n

When and Why Percent Recovery Matters<\/h3>\n

Percent recovery is important in labs and factories. In labs, it helps scientists see how good their methods are. It shows where they can get better.<\/p>\n

Laboratory Applications<\/h4>\n

In labs, percent recovery checks if experiments like recrystallization<\/strong> and chromatography<\/strong> are successful. A high percent recovery means the experiment went well. But a low one might mean there were mistakes or not enough efficiency.<\/p>\n

In factories, percent recovery is vital for making things better and wasting less. By getting more percent recovery, factories can save money and work more efficiently.<\/p>\n

Knowing and using percent recovery is key for getting the best results in labs and factories.<\/p>\n

The Difference Between Percent Recovery and Percent Yield<\/h2>\n

Percent recovery and percent yield are key terms in chemistry. They are related but have different uses. Knowing their differences helps chemists and researchers see how well their methods work.<\/p>\n

Conceptual Distinctions<\/h3>\n

Percent recovery shows how much of a substance is found after a process, like purification. It tells us how well the process worked. Percent yield, on the other hand, shows how well a chemical reaction worked. It compares the actual product to what was expected.<\/p>\n

Percent recovery is for getting substances back, while percent yield checks how good a reaction was.<\/p>\n

Practical Applications of Each Metric<\/h3>\n

Percent recovery is key in solvent extraction<\/strong> and recrystallization<\/strong>. It helps get as much substance as possible. Percent yield is important in making new substances. It shows how efficient a reaction was and where to improve.<\/p>\n

When to Use Which Calculation<\/h3>\n

Choosing between percent recovery and percent yield depends on the situation. Use percent recovery for getting substances back. Use percent yield for checking how good a reaction was.<\/p>\n

In short, percent recovery and percent yield are both vital in chemistry. But they are used for different things. Knowing the difference helps in improving chemical processes and reactions.<\/p>\n

The Mathematical Formula for Percent Recovery<\/h2>\n

To check how well a chemical process works, we need to figure out the percent recovery. This is key to knowing how much of what we want is left after a process like cleaning or making something new.<\/p>\n

Breaking Down the Percent Recovery Equation<\/h3>\n

The percent recovery formula<\/b> is simple: Percent Recovery = (Recovered Amount \/ Initial Amount) * 100<\/strong>. This formula is basic but very important in science.<\/p>\n

Mass-Based Recovery Calculations<\/h4>\n

In mass-based recovery, we measure stuff by how heavy it is. For example, when purifying something, we weigh it before and after.<\/p>\n

Mole-Based Recovery Calculations<\/h4>\n

Mole-based recovery is about counting the number of particles. This is handy when we know exactly how much of something will react.<\/p>\n

Units and Measurement Considerations<\/h3>\n

It’s important to use the same units when figuring out percent recovery. Whether it’s by weight or by number of particles, both amounts must match. Keeping measurements consistent is essential for accurate results<\/em>.<\/p>\n

Knowing how to use the percent recovery formula<\/b> is critical in chemistry. By calculating it right, scientists can see how well their methods are working and tweak them if needed.<\/p>\n

Step-by-Step Guide to Calculating Percent Recovery<\/h2>\n

To see how well a chemical reaction or process works, you need to calculate percent recovery. This is key to knowing how efficient different lab methods and processes are.<\/p>\n

Determining the Initial Amount<\/h3>\n

The first thing to do is figure out how much of the substance or product you start with. You measure or calculate this before the process or reaction starts. Getting this measurement right<\/strong> is very important for good results.<\/p>\n

Measuring the Recovered Amount<\/h3>\n

Once the process or reaction is done, you need to measure how much substance you got back. You might use methods like filtration, distillation, or extraction. Being precise<\/em> in this step is essential for a reliable percent recovery value.<\/p>\n

Performing the Calculation<\/h3>\n

To find the percent recovery, use the formula: (Recovered Amount \/ Initial Amount) * 100. This simple formula helps you see how well the process worked.<\/p>\n

Worked Example with Solution<\/h4>\n

For example, say you started with 10 grams of a substance and got 8 grams back after purification. The percent recovery would be: (8 \/ 10) * 100 = 80%. So, 80% of the initial substance was recovered.<\/p>\n\n\n\n\n\n
Initial Amount (g)<\/th>\nRecovered Amount (g)<\/th>\nPercent Recovery (%)<\/th>\n<\/tr>\n
10<\/td>\n8<\/td>\n80<\/td>\n<\/tr>\n
20<\/td>\n16<\/td>\n80<\/td>\n<\/tr>\n
5<\/td>\n4<\/td>\n80<\/td>\n<\/tr>\n<\/table>\n

By following these steps and making sure your measurements are accurate, researchers can find the percent recovery. This helps them see how efficient their processes are. Making sure you get as much back as possible is a big goal in chemical processes. Knowing how to calculate percent recovery is a key part of reaching this goal.<\/p>\n

What is Percent Yield in Chemistry?<\/h2>\n

Percent yield is key for chemists to check and improve chemical processes. It shows how much product is made compared to the maximum possible.<\/p>\n

Theoretical vs. Actual Yield<\/h3>\n

Theoretical yield is based on the reaction’s stoichiometry, assuming no losses. Actual yield is what’s really made after the reaction and product isolation.<\/p>\n

There can be big differences between theoretical and actual yield. This is because of side reactions, incomplete reactions, and losses during product isolation.<\/p>\n

The Significance of Percent Yield in Reaction Assessment<\/h3>\n

Percent yield is vital for judging chemical reaction success. It helps chemists:<\/p>\n

    \n
  • Check if a reaction worked well<\/li>\n
  • Find ways to get better results<\/li>\n
  • See which methods are more efficient<\/li>\n<\/ul>\n

    Stoichiometric Relationships<\/h4>\n

    Percent yield calculations depend on knowing the chemical reaction’s stoichiometry. This means balancing equations and finding the limiting reagent.<\/p>\n

    Limiting Reagent Considerations<\/h4>\n

    The limiting reagent is the first to run out, setting the product’s maximum amount. Knowing this is key for calculating theoretical and percent yield.<\/p>\n

    By grasping percent yield, chemists can make reactions more efficient. This leads to better and cheaper chemical processes.<\/p>\n

    The Mathematical Formula for Percent Yield<\/h2>\n

    To check how well a chemical reaction works, we need to find the percent yield. This key number shows how much product we really get compared to what we could get.<\/p>\n

    Understanding the Percent Yield Equation<\/h3>\n

    The percent yield formula is: Percent Yield = (Actual Yield \/ Theoretical Yield) * 100<\/em>. It’s key for judging a reaction’s success. The actual yield<\/strong> is what we really get. The theoretical yield<\/strong> is the most we could get based on the reactants.<\/p>\n

    Common Units and Conversions<\/h3>\n

    When we calculate percent yield, we must use the same units. This might mean changing grams to moles.<\/p>\n

    Mass to Mole Conversions<\/h4>\n

    To change mass to moles, we use: moles = mass \/ molar mass<\/em>. This is important because reactions are balanced in moles, not mass.<\/p>\n

    Handling Different Units<\/h4>\n

    Sometimes, actual and theoretical yields are in different units. For example, actual yield might be in grams, but theoretical yield in moles. We must convert both to the same unit before we can calculate percent yield.<\/p>\n

    Let’s say actual yield is 25 grams and theoretical yield is 0.5 moles. First, we convert the theoretical yield to grams. If the molar mass is 100 g\/mol, then 0.5 moles is 50 grams. The percent yield is then (25 \/ 50) * 100 = 50%.<\/p>\n

    By using the percent yield formula right, chemists can make their reactions better. They can get more product and make their work more efficient.<\/p>\n

    Step-by-Step Guide to Calculating Percent Yield<\/h2>\n

    Calculating percent yield is key in chemistry. It shows how well a reaction works. Knowing how to find percent yield is important for improving chemical processes.<\/p>\n

    Determining Theoretical Yield<\/h3>\n

    Theoretical yield is the most product you can get from a reaction. It’s based on the reaction’s balance. To find it, you need to do stoichiometric calculations.<\/p>\n

    Stoichiometric Calculations<\/h4>\n

    Stoichiometric calculations use a balanced chemical equation. They find the mole ratio between reactants and products. This ratio helps calculate the theoretical yield.<\/p>\n

    For example, in the reaction 2A + 3B \u2192 C, use 2 moles of A and 3 moles of B. Then, calculate the theoretical yield of C based on the mole ratio from the balanced equation.<\/p>\n

    Limiting Reagent Analysis<\/h4>\n

    In many reactions, one reactant is not enough. This reactant is called the limiting reagent. It decides the maximum product amount.<\/p>\n

    To find the limiting reagent, compare the mole ratio of reactants used to the balanced equation’s ratio. The reactant with the least amount is the limiting reagent.<\/p>\n\n\n\n\n
    Reactant<\/th>\nMoles Used<\/th>\nStoichiometric Coefficient<\/th>\nLimiting Reagent?<\/th>\n<\/tr>\n
    A<\/td>\n2<\/td>\n2<\/td>\nNo<\/td>\n<\/tr>\n
    B<\/td>\n1.5<\/td>\n3<\/td>\nYes<\/td>\n<\/tr>\n<\/table>\n

    Measuring Actual Yield<\/h3>\n

    The actual yield is the product you get from the reaction. You can measure it by weighing or using spectroscopy.<\/p>\n

    For yield optimization<\/strong>, aim for the actual yield to be close to the theoretical yield. Any difference means there are inefficiencies in the reaction.<\/p>\n

    “The actual yield is often less than the theoretical yield due to various factors such as side reactions, incomplete reactions, and loss of product during purification.”<\/p><\/blockquote>\n

    Performing the Calculation<\/h3>\n

    The percent yield formula is: (Actual Yield \/ Theoretical Yield) * 100%. This shows how efficient the reaction was.<\/p>\n

    For example, if the actual yield is 80 grams and the theoretical yield is 100 grams, the percent yield is (80\/100) * 100% = 80%. This means the reaction was 80% efficient.<\/p>\n

    By following these steps, chemists can improve their reactions. This leads to better recovery enhancement<\/strong> and efficiency.<\/p>\n

    Common Factors Affecting Percent Recovery<\/h2>\n

    It’s important to know what affects percent recovery in chemical processes. Percent recovery is a key metric in chemistry. It’s influenced by physical, chemical, and procedural factors.<\/p>\n

    Physical Limitations<\/h3>\n

    Physical limitations are a big part of percent recovery. These can be things like transfer losses and solubility issues.<\/p>\n

    Transfer Losses<\/h4>\n

    Transfer losses happen when moving substances between containers. These losses can really affect percent recovery, more so with small amounts. Minimizing transfer losses<\/strong> is key for recovery improvement<\/em>.<\/p>\n

    Solubility Issues<\/h4>\n

    Solubility issues also play a role. How well a substance dissolves in a solvent can limit recovery. Knowing the solubility of substances is important for better recovery.<\/p>\n

    Chemical Interferences<\/h3>\n

    Chemical interferences, like side reactions and product degradation, can also affect percent recovery. These can change the chemical makeup of the sample, making recovery harder.<\/p>\n

    Procedural Variables<\/h3>\n

    Procedural variables, like the method used, equipment, and conditions, also matter. Improving these can boost process efficiency<\/strong> and recovery rates.<\/p>\n

    In summary, percent recovery is shaped by physical, chemical, and procedural factors. By understanding and tackling these, chemists can find ways to improve percent recovery. This leads to more efficient chemical processes.<\/p>\n

    Common Factors Affecting Percent Yield<\/h2>\n

    Knowing what affects percent yield is key for better chemical reactions. Percent yield shows how efficient a chemical reaction is. Several factors can change this number. By managing these, chemists can get better results.<\/p>\n

    Side Reactions and Competing Pathways<\/h3>\n

    Side reactions and competing pathways are big factors. These unwanted reactions use up reactants, lowering the desired product. Reducing side reactions<\/strong> is vital for better percent yield. This can be done by adjusting reaction conditions and using the right catalysts.<\/p>\n

    Reaction Conditions and Their Impact<\/h3>\n

    Reaction conditions, like temperature and pressure, greatly affect percent yield. Temperature<\/em> is very important. It can change how fast a reaction happens and what by-products are formed.<\/p>\n

    Temperature Effects<\/h4>\n

    Higher temperatures speed up reactions but might damage reactants or products. Lower temperatures slow reactions down, which can help selectivity. Finding the right temperature is essential for high percent yield.<\/p>\n

    Pressure Considerations<\/h4>\n

    Pressure is also very important, mainly in gas reactions. Higher pressure<\/strong> can push reactions towards products, improving percent yield, based on Le Chatelier’s principle.<\/p>\n

    Purity of Reactants<\/h3>\n

    The purity of reactants is another big factor. Impurities can cause side reactions or mess with the main reaction, lowering yield. So, making sure reactants are pure<\/em> is critical for high percent yields.<\/p>\n

    By understanding and managing these factors, chemists can make chemical reactions more efficient. This leads to higher percent yields and more successful experiments.<\/p>\n

    Practical Examples of Percent Recovery Calculations<\/h2>\n

    The accuracy of lab results depends on percent recovery. It’s a key metric for chemists to check their technique’s efficiency.<\/p>\n

    Example 1: Solvent Extraction<\/h3>\n

    Solvent extraction separates substances based on solubility. To find percent recovery, you need to know the initial amount and the amount recovered.<\/p>\n

    For example, if 10 grams of a compound were there and 8 grams were recovered, the percent recovery is (8\/10) * 100 = 80%. This shows 80% of the compound was recovered.<\/p>\n

    Example 2: Recrystallization<\/h3>\n

    Recrystallization purifies substances. The percent recovery is calculated like solvent extraction. If a chemist starts with 5 grams and recovers 4 grams, the percent recovery is (4\/5) * 100 = 80%.<\/p>\n

    Example 3: Distillation<\/h3>\n

    Distillation separates components by boiling points. To find percent recovery, compare the collected distillate to the initial amount.<\/p>\n

    For example, if 12 grams were distilled and 9 grams were collected, the percent recovery is (9\/12) * 100 = 75%.<\/p>\n

    Troubleshooting Low Recovery Rates<\/h4>\n

    Low percent recovery can happen for many reasons. These include incomplete extraction or purification<\/strong>, decomposition of the substance<\/em>, or losses during transfer<\/strong>. Chemists should review their methods, check for losses, and improve their techniques.<\/p>\n

    Understanding and using percent recovery calculations helps chemists improve their lab work. This leads to more accurate and reliable results.<\/p>\n

    Practical Examples of Percent Yield Calculations<\/h2>\n

    To make chemical processes better, knowing how to calculate percent yield is key. Percent yield shows how well a chemical reaction works by comparing what’s made to what should be made. This is very important in the chemical industry to make more and waste less.<\/p>\n

    Synthesis Reaction<\/h3>\n

    In synthesis reactions, different substances combine to make one product. For example, nitrogen (N2<\/sub>) and hydrogen (H2<\/sub>) mix to make ammonia (NH3<\/sub>): N2<\/sub> + 3H2<\/sub> \u2192 2NH3<\/sub>. First, find the theoretical yield based on the limiting reactant. Then, measure the actual yield from the experiment.<\/p>\n

    Example Calculation:<\/strong> If ammonia’s theoretical yield is 100 grams but the actual yield is 85 grams, the percent yield is (85 \/ 100) * 100 = 85%. This shows the reaction is efficient, making 85% of what it should.<\/p>\n

    Precipitation Reaction<\/h3>\n

    Precipitation reactions make an insoluble product. For example, silver nitrate (AgNO3<\/sub>) and sodium chloride (NaCl) mix to make silver chloride (AgCl): AgNO3<\/sub> + NaCl \u2192 AgCl + NaNO3<\/sub>. The percent yield can be affected by how complete the reaction is and how well the product is filtered.<\/p>\n

      \n
    • Determine the theoretical yield of AgCl based on the reaction’s stoichiometry.<\/li>\n
    • Measure the actual yield of AgCl after it’s filtered and dried.<\/li>\n
    • Calculate the percent yield to see how efficient the reaction is.<\/li>\n<\/ul>\n

      Redox Reaction<\/h3>\n

      Redox reactions involve electron transfer between substances. For example, copper (Cu) and silver nitrate (AgNO3<\/sub>) react: Cu + 2AgNO3<\/sub> \u2192 Cu(NO3<\/sub>)2<\/sub> + 2Ag. The percent yield in redox reactions can be influenced by the reactants’ surface area and the presence of catalysts.<\/p>\n

      Analyzing Less-Than-Ideal Yields<\/h4>\n

      If the percent yield is less than 100%, the reaction isn’t perfect. Reasons include side reactions, incomplete reactions, and product loss. By understanding these, chemists can improve the reaction conditions to get better yields.<\/p>\n

      For instance<\/em>, a 70% yield means 30% of reactants were lost. By fixing these issues, chemists can make their processes more efficient and cost-effective.<\/p>\n

      Percent yield calculations help chemists make chemical reactions better. This is key in industry to save costs and protect the environment. Making processes more efficient is essential for sustainability.<\/p>\n

      Strategies for Optimizing Percent Recovery in Laboratory Procedures<\/h2>\n

      To get the most out of lab work, you need to improve your techniques, pick the right tools, and make your processes better. This means focusing on better methods and equipment.<\/p>\n

      Technique Refinement<\/h3>\n

      Improving your lab techniques is key to better recovery. It’s about reducing losses<\/strong> and making separation better<\/strong>.<\/p>\n

      Minimizing Transfer Losses<\/h4>\n

      Losses during transfer can hurt your recovery rates. To cut down on these losses, make sure to rinse your equipment well. Also, use the right containers for moving samples.<\/p>\n

      Optimizing Separation Methods<\/h4>\n

      Methods like chromatography and distillation are vital for recovery. To get the best results, choose the right columns, solvents, and temperatures.<\/p>\n

      Equipment Selection<\/h3>\n

      The tools you use matter a lot for recovery. Pick equipment that fits the job, like top-notch centrifuges and precise balances.<\/p>\n

      Process Optimization<\/h3>\n

      Improving your lab’s workflow is another way to boost recovery. This means making your procedures smoother, cutting down on handling steps, and adding quality checks.<\/p>\n\n\n\n\n\n
      Strategy<\/th>\nDescription<\/th>\nImpact on Percent Recovery<\/th>\n<\/tr>\n
      Technique Refinement<\/td>\nImproving laboratory techniques to minimize losses and optimize separation<\/td>\nHigh<\/td>\n<\/tr>\n
      Equipment Selection<\/td>\nChoosing the right equipment for the task<\/td>\nMedium<\/td>\n<\/tr>\n
      Process Optimization<\/td>\nStreamlining laboratory workflows to reduce losses and improve efficiency<\/td>\nHigh<\/td>\n<\/tr>\n<\/table>\n

      By using these strategies, lab workers can greatly improve recovery rates. This makes lab work more efficient and cost-effective.<\/p>\n

      Strategies for Improving Percent Yield in Chemical Reactions<\/h2>\n

      To get the most out of chemical reactions, several strategies can help. Making the right adjustments to reaction conditions is key.<\/p>\n

      Reaction Condition Optimization<\/h3>\n

      Changing temperature, pressure, and reaction time<\/strong> can greatly affect the yield. For example, higher temperatures can speed up reactions. But too much heat can cause unwanted side reactions. Also, adjusting pressure can change the reaction’s balance and yield.<\/p>\n

      Catalyst Selection<\/h3>\n

      The choice of catalyst<\/em> is very important. Catalysts help reactions happen faster by lowering the energy needed. This can lead to a higher percent yield.<\/p>\n

      Reactant Purity and Stoichiometry<\/h3>\n

      It’s vital to have pure reactants<\/strong> and the right stoichiometry<\/strong>. Impurities can cause side reactions, lowering the yield. And the wrong amounts can mean reactions don’t go to completion.<\/p>\n

      Green Chemistry Approaches<\/h4>\n

      Using green chemistry<\/em> can also boost percent yield. Methods like renewable feedstocks, waste reduction, and efficient pathways<\/strong> improve yield and are better for the environment.<\/p>\n

      By applying these strategies, chemists can greatly increase the percent yield of chemical reactions. This leads to more efficient and eco-friendly processes.<\/p>\n

      Conclusion: Mastering Recovery and Yield Calculations for Better Chemical Processes<\/h2>\n

      Learning about percent recovery and percent yield is key for better chemical processes. Chemists can check how well their lab work and reactions are going. Percent recovery shows how good purification methods are. Percent yield tells if chemical reactions were successful.<\/p>\n

      To get better at these, chemists need to know what affects them. They can improve by tweaking reaction settings, choosing the right tools, and perfecting methods. This boosts the success of chemical work.<\/p>\n

      This article helps readers understand percent recovery and yield better. With this knowledge, they can make smarter choices in labs and factories. This leads to more efficient and successful chemical processes.<\/p>\n","protected":false},"excerpt":{"rendered":"

      Learn how to calculate Percent Recovery and Percent Yield, essential metrics for evaluating chemical reactions.<\/p>\n","protected":false},"author":1,"featured_media":891,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[8],"tags":[255,251,249,253,252,248,254,256,250],"class_list":["post-890","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-discovery","tag-analytical-chemistry","tag-chemical-reactions","tag-chemistry-calculations","tag-chemistry-experiments","tag-laboratory-techniques","tag-percent-recovery-calculation","tag-recovery-efficiency","tag-stoichiometry","tag-yield-calculation"],"_links":{"self":[{"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/posts\/890","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/comments?post=890"}],"version-history":[{"count":1,"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/posts\/890\/revisions"}],"predecessor-version":[{"id":892,"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/posts\/890\/revisions\/892"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/media\/891"}],"wp:attachment":[{"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/media?parent=890"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/categories?post=890"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/blog.ajsrp.com\/en\/wp-json\/wp\/v2\/tags?post=890"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}