Answer :
Answer: Work done for the process is -390 J
Explanation:
The chemical equation for the reaction of zinc metal with sulfuric acid follows:
[tex]Zn+H_2SO_4\rightarrow ZnSO_4+H_2[/tex]
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Given mass of zinc = 10.0 g
Molar mass of zinc = 65.38 g/mol
Putting values in above equation, we get:
[tex]\text{Moles of zinc}=\frac{10.0g}{65.38g/mol}=0.153mol[/tex]
The equation given by ideal gas follows:
[tex]P\Delta V=nRT[/tex]
where, P = pressure of the gas
[tex]\Delta V[/tex] = Change in volume of the gas
T = Temperature of the gas = 298 K
R = Gas constant = 8.314 J/mol.K
n = number of moles of gas = 0.153 mol
Putting values in above equation, we get:
[tex]P\Delta V=0.153mol\times 8.314J/mol.K\times 298K\\\\P\Delta V=397J[/tex]
To calculate the work done, we use the equation:
[tex]\text{Work done}=-P\Delta V\\\\W=-390J[/tex]
Hence, work done for the process is -390 J