**Title: Calculating Percent Yield in a Chemical Reaction****Introduction:**This example illustrates how to calculate the percent yield of a chemical reaction. We are examining the reaction of hydrazine (\( \text{N}_2\text{H}_4 \)) with oxygen, which produces nitrogen gas (\( \text{N}_2 \)) and water (\( \text{H}_2\text{O} \)).**Chemical Equation:**\[ \text{N}_2\text{H}_4 (\text{aq}) + \text{O}_2 (\text{g}) \rightarrow \text{N}_2 (\text{g}) + 2 \text{H}_2\text{O} (\text{l}) \]**Problem Statement:**Given that 3.25 g of \( \text{N}_2\text{H}_4 \) reacts with excess oxygen and produces 0.750 L of \( \text{N}_2 \) at 295 K and 1.00 atm, determine the percent yield of the reaction.**Calculation:**To calculate the percent yield, you will first need to:1. Calculate the theoretical yield of \( \text{N}_2 \) based on the initial amount of \( \text{N}_2\text{H}_4 \).2. Use the ideal gas law (PV = nRT) to find the moles of \( \text{N}_2 \) produced and the theoretical moles that should have been produced.3. Finally, compare the actual yield to the theoretical yield to find the percent yield.**Formula:**\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\% \]**Percent Yield Box:**The calculated percent yield should be entered in the provided box.\[ \text{Percent Yield:} \ \ \ \ \square \ \% \]

The expression of ideal gas equation is shown below: PV = nRT Where; P = pressure V = volume n = moles T = temperatureGiven information: Mass of N2H4 = 3.25 g Volume of N2 = 0.750 L pressure = 1 atm Temperature = 295KThe given reaction is shown below: N2H4 + O2 → N2 + 2H2OThe calculation of moles of N2 is shown below: PV = nRTn = PVRT= 1 ×0.7500.0821 ×295= 0.0309 mol The calculation of moles of N2H4 is shown below: moles of N2H4 = Given mass of N2H4 molar mass of N2H4 =3.25 g 32 gmol-1=0.1015 molAccording to the reaction; the stoichiometry ratio of N2H4 and N2 is 1:1 So, Theoretical yield is 0.1015 mol The calculation of percent yield is shown below: percent yield = actual yieldTheoretical yield ×100= 0.03090.1015×100=30.44 %Answer: percent yield is 30.44 %

Science

Chemistry

Hydrazine, N, H,, reacts with oxygen to form nitrogen gas and water. N,H, (aq) + O,(g)→ N,(g) + 2 H,O(1) If 3.25 g of N,H, reacts with excess oxygen and produces 0.750 L of N,, at 295 K and 1.00 atm, what is the percent yield of the reaction? percent yield: %

Hydrazine, N, H,, reacts with oxygen to form nitrogen gas and water. N,H, (aq) + O,(g)→ N,(g) + 2 H,O(1) If 3.25 g of N,H, reacts with excess oxygen and produces 0.750 L of N,, at 295 K and 1.00 atm, what is the percent yield of the reaction? 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...

See similar textbooks

Similar questions

v Al(s) + Cl2(g)→ AICI3(s) v Na(s) + v N2(g) → v NazN(s) v C2H4(g) + v 02(g) - CO2(g) + v H20(g) QUESTION 7 What is the molar mass of C12H1802 in g/mole? QUESTION 8 v Law states that for a fixed amount of gas at a Click Save and Submit to save and submit. Click Save All Answers to saVE search
Given the ynbalanced equation: H2SO4 + NAOH --> BaSO4 + H2O How many moles of NaOH will react with 22.2 mol ofH,SO,?
Consider the following reaction at STP: 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g) How many moles of S will form when 4 moles of H2S reacts with 1.5 moles of SO2?Identify the limiting reagent: Identify the excess reagent:How many moles of the excess reagent will remain after the reaction is finished?
How many moles of gas would be produced if 0.0595mol of sodium bicarbonate reacted completely with acetic acid,
given that 4 NH3 + 5O2 -> 4NO + 6H2O if 3.00 mol NH3 were made to react with excess of oxygen gas, the amount of H2O formed would be?
Consider the following reaction: 2H₂ + O₂ --> 2H₂O How many moles of water can be formed from 2.5 mole of H₂ and 2.7 moles of O₂? Your Answer: 2 Answer moles of v units
Ke lo %24 3. Ss I u b 2 4. #3 5 9. 7. 8. 6. IIO mol NO How many moles of NO are formed from 2.1 moles of N,? Use the balanced equation for the reaction of N, and O, to form NO to answer the question. (6)0 + (6)N Enter your answer in the provided box. → 2 NO(g)
Given the following reaction: C3H8 + 5O2 = 3CO2 + 4H2O Using dimensional analysis: You want to form 50.0 g of water. What is the minimum number of moles of C3H8 and O2 needed?