Asked by Jamie
Hydrogen gas (H2) is generated by the following reaction.
Ca(s) + 2 HCl(aq) → CaCl2(aq) + H2(g);
ΔH = −542.7 kJ/mol
When this reaction takes place in a cylinder (fitted with a piston) containing 1.000 mol Ca(s), 542.7 kJ heat is lost to the surroundings. Because a gas is generated, work is done by the system against a constant pressure of 1.140 atm. If the internal energy decreases by 545.53 kJ,
what is the change in the volume of the system in liters?
Ca(s) + 2 HCl(aq) → CaCl2(aq) + H2(g);
ΔH = −542.7 kJ/mol
When this reaction takes place in a cylinder (fitted with a piston) containing 1.000 mol Ca(s), 542.7 kJ heat is lost to the surroundings. Because a gas is generated, work is done by the system against a constant pressure of 1.140 atm. If the internal energy decreases by 545.53 kJ,
what is the change in the volume of the system in liters?
Answers
Answered by
DrBob222
dE = q + w
Substitute dE and q and solve for w (in joules).
Convert to L*atm knowing that 1 L*atm = 101.325 J.
Then w = -pdV and solve for dV.
Substitute dE and q and solve for w (in joules).
Convert to L*atm knowing that 1 L*atm = 101.325 J.
Then w = -pdV and solve for dV.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.