### Chemistry: Understanding Reactants, Mass, and Yield1. **What is a limiting reactant? Excess reactant?** - In a chemical reaction, a limiting reactant is the substance that is totally consumed first and limits the extent of the reaction, determining the amount of product formed. An excess reactant is the substance that is present in a quantity greater than necessary to react with the limiting reactant, meaning there is some left over after the reaction is complete.2. **Why do we use the “constant mass” of NaCl in the experiment, and not the average mass?** - Using the "constant mass" of NaCl ensures accuracy and precision. It involves heating the sample to remove all moisture and allows it to cool in a desiccator, repeating the process until the mass remains constant. This eliminates errors due to moisture absorption, providing a more accurate measurement than using an average mass, which can vary due to external factors.3. **What is the name of the chemical product at the end of both reactions? Is the mass of the chemical product you measure considered the actual yield or the theoretical yield?** - The name of the chemical product will depend on the specific reactions being conducted. The mass measured in an experiment usually represents the actual yield, which is the amount of product obtained. This can differ from the theoretical yield, which is the calculated maximum amount of product that could be formed from the given quantities of reactants.4. **What is the percent yield of a reaction that produces 10.5 g CF₂Cl₂ from 29.9 g of CCl₄ and excess HF?** - The reaction is as follows: \[ \text{CCl}_4(\text{l}) + 2 \text{HF}(\text{aq}) \rightarrow \text{CF}_2\text{Cl}_2(\text{g}) + 2 \text{HCl}(\text{aq}) \] - To find the percent yield, first calculate the theoretical yield of CF₂Cl₂ based on the limiting reactant, CCl₄. Then, use the formula: \[ \text{Percent Yield} = \left(\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\right) \times 100\% \] - (Calculations would require additional data such as molar masses).

Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

Answered: 1. What is a limiting reactant? Excess…

Science

Chemistry

1. What is a limiting reactant? Excess reactant?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Balance the following reaction _____ C5H10O + _____O2 -------> _____CO2 + _____ H2O
What are 5 ways to identify chemical reaction?
A pile of leaves is lit on fire, and then covered completely with a fire blanket so that the fire goes out. Identify the limiting reactant in this situation.
Balance the following reactions _____ C6H6 + _____ O2 ---> _____ CO2 + _____ H2O
A common demonstration in chemistry courses involves adding a tiny speck of magnesium(IV) oxide to a concentrated hydrogen peroxide H2O2 solution Hydrogen peroxide is unstable and it decomposes quite spectacularly under these conditions to produce get oxygen gas and steam magnesium (IV) oxide is a catalyst for the decomposition of hydrogen peroxide and is not consumed in the reaction she was the balance equation for the decomposition reaction of hydrogen peroxide
3. A student mixes 100.0 mL of a 0.100 M solution of potassium phosphate with 100.0 mL of a 0.125 M solution of copper (II) sulfate and obtains a blue solid. (a) Write the balanced chemical equation for the reaction including physical states. (b) Determine the limiting reagent. (c) Calculate the number of moles of the excess reagent after the reaction is completed. Record servation
If the theoretical yield of a reaction is 14. 2 g and the actual yield is 7.81 grams, the percent yield is... 71.1% 182% 55.0% 100.%
Please don't provide handwritten solution .... Help me.
Stoichiometry Below is the generic skeleton chemical equation for a combustion reaction. A,B + C2 -> AC2 + B,C 1. What is the balanced equation for the combustion reaction?
Vocabulary Assignment: Quantity Relationships in Chemical Reactions 1. Stoichiometry - 2. Give an example of a balanced equation to show how to obtain conversion factors - 3. Write a stepwise mass to mass conversion for calculating mass of desired or wanted chemical given the mass of one chemical the balanced chemical equation - 4. What is the theoretical yield and how is it calculated? - 5. What is the actual or experimental yield? - 6. Write the formula for the percent yield why is this number important?- 7. Limiting reactant - 8. Use the comparison of calculated mass method to determine limiting reactan - 9. Excess reactant - 10. energy - 11. Joule - 12. Calorie - 13. Enthalpy of reactions and its relationship to exothermic and endothermic reactions- 14. Write a stepwise mass to energy conversion using a thermochemical equation to calculate energy of a reaction - short and sweet please! thank you!