1. 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. 2H2O2 (l) --> 2H2O (l) + 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.
1.
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.
2H2O2 (l) --> 2H2O (l) + 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.
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