# Question ef6c6

Jul 14, 2015

Volume: 12 L.

#### Explanation:

In order to determine the volume occupied by 1 g of hydrogen gas, ${H}_{2}$, at NTP, you must use the ideal gas law equation.

$P V = n R T \implies V = \frac{n R T}{V}$

Before using this equation to solve for $V$, you must first determine how many moles are found in 1 g of hydrogen gas. To do that, use hydrogen gas' molar mass

1cancel("g") * ("1 mole "H_2)/(2.0159cancel("g")) = "0.4961 moles"# ${H}_{2}$

Normal Temperature and Pressure (NTP) conditions imply a pressure of 1 atm and a temperature of ${20}^{\circ} \text{C}$.

Plug in your values into the ideal gas law equation to get

$V = \left(0.4961 \cancel{\text{moles") * 0.082(cancel("atm") * "L")/(cancel("mol") * cancel("K")) * (273.15 + 20)cancel("K"))/(1cancel("atm}}\right)$

$V = \text{11.9 L}$

I'll leave the answer rounded to two sig figs, despite the fact that you only gave one sig fig for the mass of hydrogen gas

$V = \textcolor{g r e e n}{\text{12 L}}$