Answer:
If the temperature and volume ot a gas increases, the r.m.s. velocity of the molecules in the gas will be 2 times the original r.m.s. molecular velocity.
If T doubles while V is held constant, the new net internal energy of the gas will be 2 times the original internal energy of the gas.
Explanation:
Temperature and root mean square velocity are directly proportional to one anoth. If the temperature increases, root mean square velocity also increases and vice versa, while temperature is also directly proportional to the internal energy of the gas molecules, higher the temperature, higher will be the internal energy and lower the temperature so internal energy will be decreased.
Answer:
Explanation:
Total mole of gases = 7.8 + 2.1 + .09 + .01 = 10
the partial pressures of the gases in a mixture
= mole fraction x Total pressure
mole fraction = mole of a gas in the mixture / total mole
partial pressure of Ng = 
= 79.014 kPa
partial pressure of O = 
= 21.273 kPa .
partial pressure of Ar = 
= .9117 kPa .
partial pressure of Co = 
= .1013 k Pa .
The last one should be right
