D,e,f,g? :) **Chemistry Problems****d)** For the equation \( \text{N}_2\text{H}_4 \rightarrow \text{NH}_3 + \text{N}_2 \), if the theoretical yield is 28.0 grams of \( \text{N}_2 \), what mass in grams of \( \text{N}_2\text{H}_4 \) would have to react?**Answer:** ___________g---**e)** For the equation \( \text{FeS} + \text{HCl} \rightarrow \text{FeCl}_2 + \text{H}_2\text{S} \), if 35.0 grams of \( \text{FeS} \) is added to 35.0 grams of \( \text{HCl} \) and allowed to react, what is the theoretical yield of \( \text{H}_2\text{S} \)?**Answer:** ___________g---**f)** Using the numbers from problem **e** above, if 10.2 grams of \( \text{H}_2\text{S} \) were obtained in the lab (actual yield), what is the percent yield?**Answer:** ___________%---**g)** How many grams of \( \text{K}_2\text{C}_2\text{O}_4 \), potassium oxalate, would contain 182 grams of pure potassium?**Answer:**

Since you have posted a question with multiple sub-parts, we will solve first three subparts for you. To get remaining sub-part solved please repost the complete question and mention the sub-parts to be solved.Given information: Theoretical yield of nitrogen = 28.0 g Mass of FeS = 35.0 g Mass of HCl = 35.0 g Actual yield of H2S = 10.2 gThe amount that is predicted by the calculation of stoichiometry of the reaction is known as theoretical yield. The amount that is produced by a product in a reaction is known as the actual yield. The ratio of actual yield to the theoretical yield is called percentage yield of a reaction.d. The balanced chemical reaction for formation of ammonia and nitrogen gas is shown below: 3N2H4→4NH3+N2According to the reaction, 1 mole of nitrogen is produced by 3 moles of N2H4 thus, the mass of N2H4 produced by Nitrogen is calculated as follows: Mass of N2H4=28.0 g N2×1 mol of N228.0134 g N2×3 mol N2H41 mol of N2× 32.0452 g N2H41 mol N2H4=96.1 g N2H4 Thus, 96.1 g of N2H4 should react.e. The balanced chemical equation for the reaction of FeS and HCl will be represented as follows: FeS+2HCl→FeCl2+H2S Now, moles of FeS and HCl are calculated as follows: Moles of FeS=Given massmolar mass=35.0 g87.91 g/mol=0.3981 molMoles of HCl=35.0 g36.46 g/mol=0.96 molAccording to the reaction, 1 mol FeS→2 mol HCl0.3981 mol FeS→2×0.3981 mol HCl0.3981 mol FeS→0.7962 mol HCl thus, 0.7962 moles of HCl are required but HCl is present in large amount that means the limiting reagent will be FeS. Thus, the amount of prouduct formed will be determined by it. According to the reaction, 1 moles of FeS gives 1 mole of H2S thus, 0.3981 moles of FeS would give 0.3981 moles of H2S. Amount of H2S=Moles×Molar mass=0.3981 mol×34.1 g/mol=13.6 g Therefore, the theoretical yield of H2S is 13.6 g.f. The percent yield of the reaction is calculated as follows: Percent yield=Actual yieldTheoretical yield×100%=10.2 g13.6 g×100%=75% Thus, the percent yield is 75%. Answer; d. The mass of N2H4 is 96.1 g. e. The theoretical yield of H2S is 13.6 g. f. The percent yield of the reaction is 75%.

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d) For the equation N2H4 → NH3 + N2, if the theoretical yield is 28.0 grams of N2, what mass in grams of N2H4, would have to react? by e) For the equation FeS + HCI → FeC2 + H2S, if 35.0g of FeS is added to 35.0g of HCl and allowed to react, what is the theoretical yield of H2S? by f) Using the numbers from problem e) above, if 10.2 g of H2S were obtained in the lab (actual yield), what is the percent yield?

d) For the equation N2H4 → NH3 + N2, if the theoretical yield is 28.0 grams of N2, what mass in grams of N2H4, would have to react? by e) For the equation FeS + HCI → FeC2 + H2S, if 35.0g of FeS is added to 35.0g of HCl and allowed to react, what is the theoretical yield of H2S? by f) Using the numbers from problem e) above, if 10.2 g of H2S were obtained in the lab (actual yield), what is the percent yield?

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...

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D,e,f,g? :)

**Chemistry Problems**

**d)** For the equation \( \text{N}_2\text{H}_4 \rightarrow \text{NH}_3 + \text{N}_2 \), if the theoretical yield is 28.0 grams of \( \text{N}_2 \), what mass in grams of \( \text{N}_2\text{H}_4 \) would have to react?

**Answer:** ___________g

---

**e)** For the equation \( \text{FeS} + \text{HCl} \rightarrow \text{FeCl}_2 + \text{H}_2\text{S} \), if 35.0 grams of \( \text{FeS} \) is added to 35.0 grams of \( \text{HCl} \) and allowed to react, what is the theoretical yield of \( \text{H}_2\text{S} \)?

**Answer:** ___________g

---

**f)** Using the numbers from problem **e** above, if 10.2 grams of \( \text{H}_2\text{S} \) were obtained in the lab (actual yield), what is the percent yield?

**Answer:** ___________%

---

**g)** How many grams of \( \text{K}_2\text{C}_2\text{O}_4 \), potassium oxalate, would contain 182 grams of pure potassium?

**Answer:**

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