When 1 mole gas is heated at constant volume, temperature is raised from 298 K to 308 K. Heat supplied to the gas is 500 J. Then which statement is correct?

Question

When 1 mole gas is heated at constant volume, temperature is raised from 298 K to 308 K. Heat supplied to the gas is 500 J. Then which statement is correct? (A) q=W=500 J, Δ U=0 (B) q=Δ U=500 J, W=0 (C) q=W= - 500 J, Δ U=0 (D) Δ U=0, q=W=-500 J

Tardigrade Admin · Accepted Answer

As we know that Δ H=Δ E +p Δ V When Δ V=0 ∴ Δ H=Δ E From first law of thermodynamics Δ U=q +W In the given problem, Δ H=500 J -W= -p Δ V, Δ V=0 So, Δ U=q=500 J

Q. When $1$ mole gas is heated at constant volume, temperature is raised from $298 K$ to $308 K$ . Heat supplied to the gas is $500 J$ . Then which statement is correct?

$q = W = 500 J, Δ U = 0$

$q = Δ U = 500 J, W = 0$

$q = W = - 500 J, Δ U = 0$

$Δ U = 0, q = W = - 500 J$

As we know that $Δ H = Δ E + p Δ V$
When $Δ V = 0$
$∴ Δ H = Δ E$
From first law of thermodynamics
$Δ U = q + W$
In the given problem, $Δ H = 500 J$
$- W = - p Δ V, Δ V = 0$
So, $Δ U = q = 500 J$

Q. When 1 mole gas is heated at constant volume, temperature is raised from 298K to 308K. Heat supplied to the gas is 500J. Then which statement is correct?

q=W=500J,ΔU=0

q=ΔU=500J,W=0

q=W=−500J,ΔU=0

ΔU=0,q=W=−500J