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FAQs on STOICHIOMETRY AND REDOX REACTIONS - Additional Documents & Tests for IIT JAM
| 1. What is stoichiometry and how is it related to redox reactions? |  |
Ans. Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves determining the amount of substances involved in a reaction based on balanced chemical equations. Redox reactions, on the other hand, are chemical reactions that involve the transfer of electrons between reactants. Stoichiometry is important in redox reactions as it allows us to calculate the amount of reactants and products involved in the electron transfer process.
| 2. How do you balance redox equations using stoichiometry? | |
Ans. Balancing redox equations involves ensuring that the number of electrons lost in the oxidation half-reaction is equal to the number of electrons gained in the reduction half-reaction. Stoichiometry can be used to balance these equations by following these steps:
1. Write the unbalanced equation for the redox reaction.
2. Split the equation into two half-reactions, one for oxidation and one for reduction.
3. Balance the atoms in each half-reaction, excluding oxygen and hydrogen.
4. Balance the oxygen atoms by adding water molecules to the half-reactions.
5. Balance the hydrogen atoms by adding H+ ions to the half-reactions.
6. Balance the charge by adding electrons to one or both of the half-reactions.
7. Multiply each half-reaction by appropriate coefficients to ensure that the number of electrons gained equals the number of electrons lost.
8. Combine the balanced half-reactions to form the overall balanced redox equation.
| 3. How can stoichiometry be used to calculate the limiting reactant in a redox reaction? | |
Ans. The limiting reactant in a redox reaction is the reactant that is completely consumed, limiting the amount of product that can be formed. Stoichiometry can be used to calculate the limiting reactant by following these steps:
1. Write the balanced chemical equation for the redox reaction.
2. Determine the moles of each reactant by dividing the given mass or volume by the molar mass or molar volume.
3. Identify the reactant with the smallest number of moles.
4. Use the balanced equation to calculate the moles of product that can be formed from each reactant.
5. The reactant with the smallest moles-to-product ratio is the limiting reactant.
| 4. How does stoichiometry help in determining the theoretical yield of a redox reaction? | |
Ans. The theoretical yield of a redox reaction is the maximum amount of product that can be formed from the limiting reactant. Stoichiometry helps in determining the theoretical yield by following these steps:
1. Write the balanced chemical equation for the redox reaction.
2. Determine the moles of the limiting reactant using stoichiometry.
3. Use the stoichiometric ratios from the balanced equation to calculate the moles of product that can be formed.
4. Convert the moles of product to grams or any other desired unit using the molar mass.
5. The calculated value is the theoretical yield of the redox reaction.
| 5. How can stoichiometry be applied to determine the percent yield of a redox reaction? | |
Ans. The percent yield of a redox reaction is the ratio of the actual yield to the theoretical yield, expressed as a percentage. Stoichiometry can be applied to determine the percent yield by following these steps:
1. Calculate the theoretical yield using stoichiometry, as explained in the previous question.
2. Perform the redox reaction and obtain the actual yield of the product.
3. Divide the actual yield by the theoretical yield and multiply by 100 to get the percent yield.
4. The percent yield indicates the efficiency of the reaction, with 100% representing a perfect conversion of the limiting reactant to the desired product.
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