70 calories of heat are required to raise the temperature of 2 moles of an ideal gas at constant pressure from 30°C to 35°C. The

Q: $70$ calories of heat are required to raise the temperature of $2$ moles of an ideal gas at constant pressure from $30°C$ to $35°C.$ The amount of heat required to raise the temperature of same gas through the same range $(30°C$ to $35°C)$ at constant volume ..... $cal$ $(R = 2 \,cal/mol/K)$

b ${(\Delta Q)_P} = \mu {C_P}\Delta T$ $\Rightarrow$ $2 \times {C_P} \times (35 - 30)$ $\Rightarrow$ ${C_P} = 7\frac{{cal}}{{mole{\rm{ - }}K}}$ $\because$ ${C_P} - {C_V} = R$ $\Rightarrow$ ${C_V} = {C_P} - R = 7 - 2 = 5\frac{{cal}}{{mole{\rm{ - }}kevin}}$ $\therefore$ ${(\Delta Q)_V} = \mu {C_V}\Delta T = 2 \times 5 \times (35 - 30) = 50\,cal.$

SECTION - A [PHYSICS MCQ]

GSEB - English Medium

$70$ calories of heat are required to raise the temperature of $2$ moles of an ideal gas at constant pressure from $30°C$ to $35°C.$ The amount of heat required to raise the temperature of same gas through the same range $(30°C$ to $35°C)$ at constant volume ..... $cal$ $(R = 2 \,cal/mol/K)$

A$30$
B$50$
C$70$
D$90$

IIT 1985, Diffcult

STD 11 Science
JEE
STD 11 - 12 . kinetic theory of gases
Physics

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