# Problem: Consider the following chemical reaction: C(s) + H2O(g) → CO(g) + H2(g). How many liters of hydrogen gas is formed from the complete reaction of 16.6 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 .

###### FREE Expert Solution

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

Step 1. mole (n) H2(g)

molar mass of C = 12.01 g/mol

C(s) + H2O(g) → CO(g) + H2(g)

1 mol of C(s) forms 1 mol H2(g)

###### Problem Details

Consider the following chemical reaction: C(s) + H2O(g) → CO(g) + H2(g). How many liters of hydrogen gas is formed from the complete reaction of 16.6 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 .