A mixture of gases contains 3.46 g of SO2, 5.53 g of H2, and 1.50 g of O2. What is the partial pressure in atm of each component of this mixture if it is held in a 56.2-L vessel at 27.7 oC? Use R = 0.0821 L-atm/mol-K as the value of the gas constant. a) P(SO2) = 0.0237 atm, P(H2) = 1.20 atm, and P(O2) = 0.0206 atm. b) P(SO2) = 0.658 atm, P(H2) = 0.412 atm, and P(O2) = 1.52 atm. c) P(SO2) = 0.306 atm, P(H2) = 0.490
A mixture of gases contains 3.46 g of SO2, 5.53 g of H2, and 1.50 g of O2. What is the partial pressure in atm of each component of this mixture if it is held in a 56.2-L vessel at 27.7 oC? Use R = 0.0821 L-atm/mol-K as the value of the gas constant. a) P(SO2) = 0.0237 atm, P(H2) = 1.20 atm, and P(O2) = 0.0206 atm. b) P(SO2) = 0.658 atm, P(H2) = 0.412 atm, and P(O2) = 1.52 atm. c) P(SO2) = 0.306 atm, P(H2) = 0.490
Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A mixture of gases contains 3.46 g of SO2, 5.53 g of H2, and 1.50 g of O2. What is the partial pressure in atm of each component of this mixture if it is held in a 56.2-L vessel at 27.7 oC? Use R = 0.0821 L-atm/mol-K as the value of the gas constant.
a) P(SO2) = 0.0237 atm, P(H2) = 1.20 atm, and P(O2) = 0.0206 atm.
b) P(SO2) = 0.658 atm, P(H2) = 0.412 atm, and P(O2) = 1.52 atm.
c) P(SO2) = 0.306 atm, P(H2) = 0.490 atm, and P(O2) = 0.133 atm.
d) P(SO2) = 8.13 atm, P(H2) = 0.160 atm, and P(O2) = 9.37 atm.
e) P(SO2) = 74.9 atm, P(H2) = 3.80e+03 atm, and P(O2) = 65.0 atm.
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