2 moles of an ideal gas expanded isothermally and reversibly from 1 L to 10 L at 300 K. What is the enthalpy change?

Question

2 moles of an ideal gas expanded isothermally and reversibly from 1 L to 10 L at 300 K. What is the enthalpy change? (A) 4.98 kJ (B) 11.47 kJ (C) -11.47 k (D) 0 kJ

Tardigrade Admin · Accepted Answer

H = E + PV Δ H =Δ E +Δ( PV ) Since, PV = nRT So, Δ H =Δ E + nR Δ T Δ T =0 and Δ E =0 ∴ Δ H =0 Enthalpy change for an ideal gas in an isothermal and reversible process is Zero.

Q. $2$ moles of an ideal gas expanded isothermally and reversibly from $1 L$ to $10 L$ at $300 K$ . What is the enthalpy change?

4.98 kJ

11.47 kJ

-11.47 k

0 kJ

$H = E + P V$
$Δ H = Δ E + Δ (P V)$
Since, $P V = n RT$
So, $Δ H = Δ E + n R Δ T$
$Δ T = 0$ and $Δ E = 0$
$∴ Δ H = 0$
Enthalpy change for an ideal gas in an isothermal and reversible process is Zero.

Q. 2 moles of an ideal gas expanded isothermally and reversibly from 1L to 10L at 300K. What is the enthalpy change?