How many moles of a gas at 104°C would occupy a volume of 6.8
L at a pressure of 270 mm Hg?

0.079mole

Explanation:

From the question given, we obtained the following data:

T = 104°C = 104 + 273 = 377K

V = 6.8L

P = 270 mmHg

Recall: 760mmHg = 1atm

Therefore, 270 mmHg = 270/760 = 0.36atm

R = 0.082atm.L/Kmol

n =?

Using the ideal gas equation:

PV = nRT

We can easily obtain the number of mole as follow:

PV = nRT

n = PV /RT

n = 0.36 x 6.8 / 0.082 x 377

n = 0.079mole

The number of mole of the gas is 0.079mole

false

because it does not have the potential to be entirely used up

if you mean hydrogen and oxygen then water is the product