Suppose 1400 J of heat are added to 1.8 mol of argon gas at a constant pressure of 120 kPa. (Assume that the argon can be treated as an ideal monatomic gas.)
(a) Find the change in internal energy. J
(b) Find the change in temperature for this gas. K
(c) Calculate the change in volume of the gas. m3
Solution:
Given:
Q = 1400 J
n = 1.8 mol
P = 120 kPa
Since: Q = (5/2) n R ΔT
1400 = (5/2)(1.8)(8.314) ΔT
ΔT = 37.42 K
The change in internal energy is : ΔU = (3/2) n R ΔT
ΔU = (3/2)(1.8 mol)(8.314)(37.42)
ΔU = 840 J
Since: Q = ΔU + W
Thus : The work done is given as : W = 1400 - 840 = 560 J
But, W = P ΔV
560 = (120 x 103 Pa) ΔV
ΔV = 0.004666 m3
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