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

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !

your parents i think this could be it