Question

1. If 1000 cal of heat is added to 4 mole of a monoatomic gas
without changing its volume, then change in temperature of
the gas is
(a) 233 K
(b) 833 K
(C) 123 K
(d) 433 K
2 The specific heat at constant pressure is greater than that of

Answer 1

Answer:

88k

Explanation:

because 1000 cal changes it to 88k

Answer 2

Answer:

(b) 833 k

Explanation:

okay let's see what's given :-

•Heat added into the system = ∆Q = 1000 cal

•The gas is monoatomic therefore "degree of freedom" will be = f = 3

Cv = f × R ÷ 2

if f = 3

therefore Cv = 3/2 × R

we know R = gas constant = 8.3

therefore Cv = 12.45 joule/ K

the value of heat is in "cal" so we need to turn "joule" into "cal" first

4.2 joule = 1 cal

12.45/4.2 = 2.9 cal

Cv = 1/n × ∆Q/∆T

∆T = 1/n × ∆Q/Cv

placing value

∆T = 1/4 × 1000/2.9

∆T = 83.3 K

(the answer is correct, the problem is that the value of heat added should be 10,000 instead of 1,000 it's either the writing mistake, or the question has been printed wrong)

if we take 10,000 cal then

∆T = 1/4 × 10000/2.9

∆T = 833 k