**Hydrogen Peroxide Decomposition Experiment**When hydrogen peroxide is decomposed in a lab, oxygen gas \((\text{O}_2)\) is collected over water at \(15.0^\circ \text{C}\). The molar masses are provided for reference: - \(\text{H}_2\text{O}_2 = 34.02 \, \text{g/mol}\) - \(\text{H}_2\text{O} = 18.02 \, \text{g/mol}\) - \(\text{O}_2 = 32.00 \, \text{g/mol}\).**Reaction Equation:**\[ 2 \, \text{H}_2\text{O}_2(l) \rightarrow 2 \, \text{H}_2\text{O}(l) + \text{O}_2(g) \]**Problem Statement:**1. **Moles of \(\text{O}_2\) Collected**: - Calculate the moles of \(\text{O}_2(g)\) collected if the total pressure of the gas is \(780 \, \text{mmHg}\) and the volume of gas is \(0.4000 \, \text{L}\). Assume all gases are ideal.2. **Volume of Decomposed \(\text{H}_2\text{O}_2\)**: - What volume of pure hydrogen peroxide \((\text{density} = 1.530 \, \text{g/mL})\) decomposed? Assume that the decomposition reaction is complete. If unable to solve part (a), assume that 1 mole of \(\text{O}_2(g)\) was collected.3. **Gas Effusion Explanation**: - If the collected gas \((\text{H}_2\text{O(g)} + \text{O}_2(g))\) is transferred into a rubber balloon (which contains tiny pores), determine which gas will effuse out more quickly. Briefly explain why your answer makes physical sense. Ignore the difference in partial pressures for this problem.**Vapor Pressure Data from Table 10.2**:The table provides the vapor pressures of water at various temperatures:- At \(15^\circ \text{C}\), the vapor pressure is \(12.8 \,

The chemical equation for the decomposition of H2O2 is: 2H2O2(l) ----> 2H2O(l) + O2(g)…

Hydrogen peroxide is decomposed in a lab and the produced O2 (g) is collected over water at 15.0 °C. Molar masses: H2O2 = 34.02 g/mol, H2O = 18.02 g/mol, O2 = 32.00 g/mol. 2 H2O2 () → 2 H20 () + O2 (g) a) Calculate the moles of O2 (g) collected if the total pressure of the gas is 780. mmHg and the volume of gas is 0.4000 L. Assume all gases are ideal. b) What volume of pure hydrogen peroxide (density = 1.530 g/mL) decomposed? Assume that the decomposition reaction is complete. If you were unable to answer part (a), assume that 1 mol of O2 (g) was collected. c) If the collected gas (H2O (g) + O2 (g)) is transferred into a rubber balloon (which contains tiny pores), which gas will effuse out more quickly? Briefly explain (in about 1 sentence) why your answer makes physical sense. You can ignore the difference in partial pressures for this problem. TABLE 10.2 VAPOR PRESSURE OF WATER TEMPERATURE ("C) PRESSURE (mm Hg) TEMPERATURE ("c) PRESSURE (mm Hg) 6.5 55 118.0 10 9.2 60 149.4 15 12.8 65 187.5 20 17.5 70 233.7 25 23.8 75 289.1 30 31.8 80 355.1 35 41.2 85 433.6 40 55.3 90 525.8 45 71.9 95 633.9

Hydrogen peroxide is decomposed in a lab and the produced O2 (g) is collected over water at 15.0 °C. Molar masses: H2O2 = 34.02 g/mol, H2O = 18.02 g/mol, O2 = 32.00 g/mol. 2 H2O2 () → 2 H20 () + O2 (g) a) Calculate the moles of O2 (g) collected if the total pressure of the gas is 780. mmHg and the volume of gas is 0.4000 L. Assume all gases are ideal. b) What volume of pure hydrogen peroxide (density = 1.530 g/mL) decomposed? Assume that the decomposition reaction is complete. If you were unable to answer part (a), assume that 1 mol of O2 (g) was collected. c) If the collected gas (H2O (g) + O2 (g)) is transferred into a rubber balloon (which contains tiny pores), which gas will effuse out more quickly? Briefly explain (in about 1 sentence) why your answer makes physical sense. You can ignore the difference in partial pressures for this problem. TABLE 10.2 VAPOR PRESSURE OF WATER TEMPERATURE ("C) PRESSURE (mm Hg) TEMPERATURE ("c) PRESSURE (mm Hg) 6.5 55 118.0 10 9.2 60 149.4 15 12.8 65 187.5 20 17.5 70 233.7 25 23.8 75 289.1 30 31.8 80 355.1 35 41.2 85 433.6 40 55.3 90 525.8 45 71.9 95 633.9

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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