If an ideal gas has volume V at 270C and it is heated at a constant pressure, so that its volume becomes 1.5 V, then the value of final temperature is:
327 K
1770C
873 K
6000C
Gas exerts pressure on the walls of the container because:
Gas has weight
Gas molecules have momentum
Gas molecules collide with each other
Gas molecules collide with the walls of the container
The temperature of a gas is raised from 270C to 9270C. What change will occur to the rms molecular speed ?
gets halved
gets doubled
gets times the earlier value
remains unchanged
the average velocity of a gas becomes 4 times, then what will be the effect on rms velocity at the same temperature?
1.4 times
4 times
3 times
2 times
If for a gas , this gas is made with which type of molecules ?
Diatomic
Mixture of diatomic and polyatomic
Monoatomic
Polyatomic
Cooking gas containers are kept in a lorry moving with uniform speed. What happend to the temperature of the gas molecules inside it ?
Increase
Decrease
Remain the same
Decrease for some, while increase for others.
A given amount of gas at 20o C has a pressure P. The temperature at which the pressure will be 2 P (at constant volume) is approximately
113o C
40o C
213o C
313o C
A monoatomic gas is suddenly compressed to (1/8)th of its initial volume adiabatically. The ratio of its final pressure to the initial pressure is (Given: the ratio of the specific heats of the given gas to be 5/3) :
32
40/3
24/5
8
When we heat a gas-sample from 270 C to 3270 C, then the initial average kinetic energy of the molecules was E. What will be the average kinetic energy?
327 E
300 E
2 E
The temperature of a given mass is increased from 270C to 3270C. The rms velocity of the molecules increases:
