Question

How many liters of hydrogen gas is formed from the complete reaction of 15.9 g c? assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 k ?

Answer 1

C + H2O -> H2 + CO
n(C) = 15.9/12 = 1.325 (mol)
=> n(H2) = 1.325 mol
We have:
PV = nRT
=> V = (nRT)/P
(R = 22.4/273 = 0.082)
V = (1.325 x 0.082 x 360)/1 = 39.114 (L)

Answer 2

Answer : The volume of hydrogen gas formed is, 39.2 liters.

Explanation :

The balanced chemical reaction is:

$C(s)+H_2O(g)\rightarrow CO(g)+H_2(g)$

First we have to calculate the moles of carbon (C).

$\text{Moles of }C=\frac{\text{Mass of }C}{\text{Molar mass of }C}$

Molar mass of carbon = 12 g/mole

Mass of carbon = 15.9 g

$\text{Moles of }C=\frac{15.9g}{12g/mole}=1.325mole$

Now we have to calculate the moles of $H_2$ gas.

From the reaction we conclude that,

As, 1 mole of carbon reaction to give 1 mole of hydrogen gas

So, 1.325 mole of carbon reaction to give 1.325 mole of hydrogen gas

Now we have to calculate the volume of hydrogen gas by using ideal gas equation.

$PV=nRT$

where,

P = Pressure of $H_2$ gas = 1.0 atm

V = Volume of $H_2$ gas = ?

n = number of moles  $H_2$ = 1.325 mole

R = Gas constant = $0.0821L.atm/mol.K$

T = Temperature of $H_2$ gas = 360 K

Putting values in above equation, we get:

$1.0atm\times V=1.325mole\times (0.0821L.atm/mol.K)\times 360K$

$V=39.2L$

Therefore, the volume of hydrogen gas formed is, 39.2 liters.