Question

When 1 mol of a gas is heated at constant
volume, temperature is raised from 298 to 308 K.
If heat supplied to the gas is 500 J, then which
statement is correct ?
(a) q = w = 500 J, ΔU = 0
(b) q = ΔU = 500 J, w = 0
(c) q = –w = 500 J, ΔU = 0
(d) ΔU = 0, q = w = –500 J

Answer 1

Answer:

The correct option is: (b) q = ΔE = 500 J,w = 0 

Explanation : ΔH = ΔE + PΔV When ΔV = 0; w = 0. As ΔE = q + w, ΔE = q In the present problem, ΔH = 500 J, ΔH = ΔE = 500 J, q = 500 J, w = 0

Answer 2

option A a) q = w = 500 J, ΔU = 0

Explanation : ΔH = ΔE + PΔV When ΔV = 0; w = 0. As ΔE = q + w, ΔE = q In the present problem, ΔH = 500 J, ΔH = ΔE = 500 J, q = 500 J, w = o