What mass of hydrogen is formed if 275 L of methane (measured at STP) is converted to synthesis gas

Methane, CH4(g), reacts with steam to give synthesis gas, a mixture of carbon monoxide and hydrogen, which is used as starting material for the synthesis of a number of organic and inorganic compounds.

CH4(g) + H2O(g) → CO(g) + 3H2(g)

What mass of hydrogen is formed if 275 L of methane (measured at STP) is converted to synthesis gas?


Can someone help me with this? I've calculated it like 10 different times and I keep getting the wrong answer. I'm not sure where I'm messing up... thanks in advance.

STP conditions are 1 atm pressure and 273 K temperature

now using PV = nRT

to calculate no.of moles of CH4

P = 1 atm
V = 275 L
n = ? moles
R = 0.0821 L atm/K/mole
T = 273 K

1 X 275 = n X 0.0821 X 273

275 = n X 22.413

n = 275/22.413 = 12.269

now 1 mole of CH4 gives 3 moles of H2

so 12.269 mole of CH4 will give 3 X 12.269 = 36.807 moles of H2

now molecular mass of H2 or weight of 1 mole of H2 = 2 g

so 36.807 moles of H2 = 36.807 X 2 = 73.614 g of H2

feel free to ask any question