105 calories of heat is required to raise the temperature of 3 moles of an ideal gas at constant pressure from 30^{circ} C to 35^{circ}

Q: $105$ calories of heat is required to raise the temperature of $3$ moles of an ideal gas at constant pressure from $30^{\circ} C$ to $35^{\circ} C$. The amount of heat required in calories to raise the temperature of the gas through the range $\left(60^{\circ} C\right.$ to $\left.65^{\circ} C \right)$ at constant volume is ........ $cal$ $\left(\gamma=\frac{C_p}{C_v}=1.4\right)$

b (b) At constant pressure heat absorbed $=\Delta Q=n C_P \Delta T \quad \dots (1)$ At constant volume heat absorbed $=\Delta U=n C_v \Delta T \quad \dots (2)$ Dividing $(1)$ by $(2)$, $\frac{\Delta Q}{\Delta U}=\frac{C_P}{C_V}=\gamma=1.4 \Rightarrow \frac{105}{\Delta U}=1.4$ $\therefore \Delta U_V=75 \,cal$

SECTION - A [PHYSICS MCQ]

GSEB - English Medium

$105$ calories of heat is required to raise the temperature of $3$ moles of an ideal gas at constant pressure from $30^{\circ} C$ to $35^{\circ} C$. The amount of heat required in calories to raise the temperature of the gas through the range $\left(60^{\circ} C\right.$ to $\left.65^{\circ} C \right)$ at constant volume is ........ $cal$ $\left(\gamma=\frac{C_p}{C_v}=1.4\right)$

A$50$
B$75$
C$70$
D$90$

Medium

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

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