A fixed number of moles of an ideal gas are kept in a container of volume V and an absolute temperature T. If T and V are both doubled, the new r. m.s. velocity of the molecules in the gas will be times the original r. m.s. molecular velocity. A: 1/4 B: 1/2 C: 1/sqrt(2) D: equal to E: sqrt(2) F: 2 G: 4 If T doubles while V is held constant, the new net internal energy of the gas will be times the original internal energy of the gas.

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.

the answer is 0.8m.

by: nicholas

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2