Law of Gases (Boyle's Law, Charles's Law, Gay-Lussac's Law, Avogadro's Law)
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NEET DIGITAL LIBRARY
Kinetic Theory of Gases

138932 A gas is at $27^{\circ} \mathrm{C}$. Its volume is doubled keeping pressure constant, then final temperature is :

1 $600^{\circ} \mathrm{C}$
2 $327 \mathrm{~K}$
3 $327^{\circ} \mathrm{C}$
4 $273^{\circ} \mathrm{C}$
JCECE-2006
Kinetic Theory of Gases

138933 Assuming the expression for the pressure exerted by the gas on the walls of the container, it can be shown that pressure is

1 $\left[\frac{1}{3}\right]^{\text {rd }}$ kinetic energy per unit volume of a gas
2 $\left[\frac{2}{3}\right]^{\text {rd }}$ kinetic energy per unit volume of a gas
3 $\left[\frac{3}{4}\right]^{\text {th }}$ kinetic energy per unit volume of a gas
4 $\frac{3}{2} \times$ kinetic energy per unit volume of a gas
MHT-CET 2015
Kinetic Theory of Gases

138935 A perfect gas at $27^{0} \mathrm{C}$ is heated at constant pressure so as to double its volume. The increase in temperature of the gas will be :

1 $600^{\circ} \mathrm{C}$
2 $327^{\circ} \mathrm{C}$
3 $54^{\circ} \mathrm{C}$
4 $300^{\circ} \mathrm{C}$
Karnataka CET-2011
Kinetic Theory of Gases

138937 70 calories of heat are required to raise the temperature of 2 moles of an ideal gas at constant pressure from $30^{\circ} \mathrm{C}$ to $35^{\circ} \mathrm{C}$. The amount of heat required in calories to raise the temperature of the same gas through the same range $\left(30^{\circ} \mathrm{C}-35^{\circ} \mathrm{C}\right)$ at constant volume is

1 $30 \mathrm{cal}$
2 $50 \mathrm{cal}$
3 $370 \mathrm{cal}$
4 $90 \mathrm{cal}$
J and K CET- 2000
Join With Us for More Updates
Kinetic Theory of Gases

138932 A gas is at $27^{\circ} \mathrm{C}$. Its volume is doubled keeping pressure constant, then final temperature is :

1 $600^{\circ} \mathrm{C}$
2 $327 \mathrm{~K}$
3 $327^{\circ} \mathrm{C}$
4 $273^{\circ} \mathrm{C}$
JCECE-2006
Kinetic Theory of Gases

138933 Assuming the expression for the pressure exerted by the gas on the walls of the container, it can be shown that pressure is

1 $\left[\frac{1}{3}\right]^{\text {rd }}$ kinetic energy per unit volume of a gas
2 $\left[\frac{2}{3}\right]^{\text {rd }}$ kinetic energy per unit volume of a gas
3 $\left[\frac{3}{4}\right]^{\text {th }}$ kinetic energy per unit volume of a gas
4 $\frac{3}{2} \times$ kinetic energy per unit volume of a gas
MHT-CET 2015
Kinetic Theory of Gases

138935 A perfect gas at $27^{0} \mathrm{C}$ is heated at constant pressure so as to double its volume. The increase in temperature of the gas will be :

1 $600^{\circ} \mathrm{C}$
2 $327^{\circ} \mathrm{C}$
3 $54^{\circ} \mathrm{C}$
4 $300^{\circ} \mathrm{C}$
Karnataka CET-2011
Kinetic Theory of Gases

138937 70 calories of heat are required to raise the temperature of 2 moles of an ideal gas at constant pressure from $30^{\circ} \mathrm{C}$ to $35^{\circ} \mathrm{C}$. The amount of heat required in calories to raise the temperature of the same gas through the same range $\left(30^{\circ} \mathrm{C}-35^{\circ} \mathrm{C}\right)$ at constant volume is

1 $30 \mathrm{cal}$
2 $50 \mathrm{cal}$
3 $370 \mathrm{cal}$
4 $90 \mathrm{cal}$
J and K CET- 2000
For More Updates join with Us
Kinetic Theory of Gases

138932 A gas is at $27^{\circ} \mathrm{C}$. Its volume is doubled keeping pressure constant, then final temperature is :

1 $600^{\circ} \mathrm{C}$
2 $327 \mathrm{~K}$
3 $327^{\circ} \mathrm{C}$
4 $273^{\circ} \mathrm{C}$
JCECE-2006
Kinetic Theory of Gases

138933 Assuming the expression for the pressure exerted by the gas on the walls of the container, it can be shown that pressure is

1 $\left[\frac{1}{3}\right]^{\text {rd }}$ kinetic energy per unit volume of a gas
2 $\left[\frac{2}{3}\right]^{\text {rd }}$ kinetic energy per unit volume of a gas
3 $\left[\frac{3}{4}\right]^{\text {th }}$ kinetic energy per unit volume of a gas
4 $\frac{3}{2} \times$ kinetic energy per unit volume of a gas
MHT-CET 2015
Kinetic Theory of Gases

138935 A perfect gas at $27^{0} \mathrm{C}$ is heated at constant pressure so as to double its volume. The increase in temperature of the gas will be :

1 $600^{\circ} \mathrm{C}$
2 $327^{\circ} \mathrm{C}$
3 $54^{\circ} \mathrm{C}$
4 $300^{\circ} \mathrm{C}$
Karnataka CET-2011
Kinetic Theory of Gases

138937 70 calories of heat are required to raise the temperature of 2 moles of an ideal gas at constant pressure from $30^{\circ} \mathrm{C}$ to $35^{\circ} \mathrm{C}$. The amount of heat required in calories to raise the temperature of the same gas through the same range $\left(30^{\circ} \mathrm{C}-35^{\circ} \mathrm{C}\right)$ at constant volume is

1 $30 \mathrm{cal}$
2 $50 \mathrm{cal}$
3 $370 \mathrm{cal}$
4 $90 \mathrm{cal}$
J and K CET- 2000
NEET DIGITAL LIBRARY
Kinetic Theory of Gases

138932 A gas is at $27^{\circ} \mathrm{C}$. Its volume is doubled keeping pressure constant, then final temperature is :

1 $600^{\circ} \mathrm{C}$
2 $327 \mathrm{~K}$
3 $327^{\circ} \mathrm{C}$
4 $273^{\circ} \mathrm{C}$
JCECE-2006
Kinetic Theory of Gases

138933 Assuming the expression for the pressure exerted by the gas on the walls of the container, it can be shown that pressure is

1 $\left[\frac{1}{3}\right]^{\text {rd }}$ kinetic energy per unit volume of a gas
2 $\left[\frac{2}{3}\right]^{\text {rd }}$ kinetic energy per unit volume of a gas
3 $\left[\frac{3}{4}\right]^{\text {th }}$ kinetic energy per unit volume of a gas
4 $\frac{3}{2} \times$ kinetic energy per unit volume of a gas
MHT-CET 2015
Kinetic Theory of Gases

138935 A perfect gas at $27^{0} \mathrm{C}$ is heated at constant pressure so as to double its volume. The increase in temperature of the gas will be :

1 $600^{\circ} \mathrm{C}$
2 $327^{\circ} \mathrm{C}$
3 $54^{\circ} \mathrm{C}$
4 $300^{\circ} \mathrm{C}$
Karnataka CET-2011
Kinetic Theory of Gases

138937 70 calories of heat are required to raise the temperature of 2 moles of an ideal gas at constant pressure from $30^{\circ} \mathrm{C}$ to $35^{\circ} \mathrm{C}$. The amount of heat required in calories to raise the temperature of the same gas through the same range $\left(30^{\circ} \mathrm{C}-35^{\circ} \mathrm{C}\right)$ at constant volume is

1 $30 \mathrm{cal}$
2 $50 \mathrm{cal}$
3 $370 \mathrm{cal}$
4 $90 \mathrm{cal}$
J and K CET- 2000
Join With Us for More Updates