A 1.00 mole sample of hydrogen gas has a temeprature of 27.0 degree celsius. The

Question

A 1.00 mole sample of hydrogen gas has a temeprature of 27.0 degree celsius. The atomic mass of hydrogen is 1.00u.

a. What is the mass of 1.00 mole of H2 gas? ZGive your answer in kg. Ans=0.00200kg

b. What is the total kinetic energy of all the gas molecules in the sample? Ans=3740J

c. If the kelvin temperature of the gas is raised by 3%, is the change in the average kinetic energy of the gas molecules less than, greater than, or equal to 3%? Justify your answer. Equal to.

d. If the temperature of the gas is raised to 90.0 degree celsius to 90.0 dedree celsius, what is the percent change in the rms speed of molecules in the gas? Ans= 10.0%

Explanation / Answer

A) Mass of one mole of H2 gas = 2 g/mol = 0.002 Kg

b) total kinetic energy = (3/2 )(nRT)

= (3/2) x1 mole x 8.314 J/K.mol. x300K

= 3741 J

c) If the temperature s raised by 3%

Kinetic energy = (3/2) (nR Tx3/100)

= 3/100(3/2nRT)

Thus the kinetic energy also increases by 3%

d) rmas speed = (3RT/M)1/2

If the temperature is increased from 90 to 190 C

Cat190/C at 90 =[ (190+273)/(90+273)]1/2

   = (463/363)1/2

= 1.12

Thus the change is 11%

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