Respuesta :
Answer
2612 mL
Explanation
Given:
The initial volume, V₁ = 300 mL
The initial pressure, P₁ = 1.2 bar
The initial temperature, T₁ = 25⁰C = (25⁰C + 273) = 298 K
The final pressure, P₂ = 0.45 bar
The final temperature, T₂ = 700⁰C = (700⁰C + 273) = 973 K
What to find:
The final volume, V₂ of the gas at 0.45 bar pressure and 700⁰C.
Step-by-step solution:
The question is a volume, pressure, and temperature relationship.
The final volume, V₂ of the gas at 0.45 bar pressure and 700⁰C can be calculated using the Combine gas law equation.
[tex]\begin{gathered} \frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2} \\ \\ V_2=\frac{P_1V_1T_2}{T_1P_2} \end{gathered}[/tex]Substituting the values of the parameters into the formula
[tex]\begin{gathered} V_2=\frac{1.2\text{ }bar\times300\text{ }mL\times973\text{ }K}{298\text{ }K\times0.45\text{ }bar} \\ \\ V_2=\frac{350280\text{ }mL}{134.1} \\ \\ V_2=2612\text{ }mL \end{gathered}[/tex]Hence, the volume of the hydrogen gas sample at 0.45 bar pressure and 700⁰C is 2612 mL.
