First, we need to use the ideal gas law to find the moles of hydrogen sulfide in the initial container:
PV = nRT
(729.6 torr)(0.0456 L) = n(0.08206 L.atm/mol.K)(298.1 K)
33.266 torr.L = 24.37n
n = 1.36 mol
Next, we need to find the new temperature in the larger container using the ideal gas law and the moles of hydrogen sulfide we calculated:
PV = nRT
(896.0 torr)(0.0699 L) = (1.36 mol)(0.08206 L.atm/mol.K)(T)
62.49 = 0.1114T
T = 561.2 K
Therefore, the temperature in the new container is 561.2 K.
Hydrogen sulfide, H,S, has the characteristic odor of rotten eggs. If a sample of H, gas at 729.6 torr and 25.1 °C in a 45.6 mL, container is allowed to enter a 69.9 mL container at a pressure of 896.0 torr, what is the temperature in the new container? Be sure your answer has the correct number of significant figures.
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1 answer