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Hydrogen gas H2 is the least dense of all gases. A sample of H2 gas is found to occupy a volume of 1.23L at 755 mmHg and 0 degrees Celsius. What volume, in liters, will this same gas occupy at .97 atm and a temperature of 50 degrees Celsius. Please indicate the equation used, variable you solved for and answer with the correct units.

User Prentice
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1 Answer

20 votes
20 votes

Answer;


1.49L

Explanations:

In order to get the required volume in liters of hydrogen, we will use the general gas equation expressed as:


(P_1V_1)/(T_1)_{}=(P_2V_2)/(T_2)_{}

P1 and P2 are the initial and final pressure of the gas

V1 and V2 are the initial and final volume of the gas

T1 and T2 are the initial and final temperatures of the gas:

Given the following parameters:


\begin{gathered} P_1=755\operatorname{mm}Hg \\ V_1=1.23L \\ T_1=0^0C=273K \\ P_2=0.97\text{atm}=737.2\operatorname{mm}Hg \\ T_2=50+273=323K_{} \\ V_2=\text{?} \end{gathered}

Substitute the given parameters into the formula as shown:


\begin{gathered} V_2=(P_1V_1T_2)/(P_2T_1) \\ V_2=\frac{755\cancel{\operatorname{mm}Hg}*1.23L*323\cancel{K}}{737.3\cancel{\operatorname{mm}Hg}*273\cancel{K}} \\ V_2=(755*1.23L*323)/(737.3*273) \\ V_2=(299,953.95)/(201282.9) \\ V_2=1.49L \end{gathered}

Hence the volume, in liters that the same gas will occupy at 0.97 atm and a temperature of 50 degrees Celsius is 1.49L

User Uamanager
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