If 57.5 mol of an ideal gas is at 4.97 atm at 69.80 ∘C, what is the volume of the gas?

325 L

Explanation:

We will use the ideal gas law: PV= nRT. Let's rearrange it so we're solving for V, so it'll instead be V=

Before we start, let's check our units. Usually it has to be the same as the units found in the constant (R)= 0.082057 L⋅atm/mol⋅K. We have temperature in Celsius here so let's convert it to Kelvin (K).

69.80C +273= 342.8 K

Now we can plug everything in.

V=

V== 325 L

n+h→nh3

we must remember that nitrogen and hydrogen are both diatomic molecules in their standard gas form. this adjusts the equation to

n2+h2→nh3

now we need to adjust coefficients in order to balance the atoms on each side of the equation. currently we have 2 atoms of nitrogen and 2 atoms of hydrogen on the reactant side and 1 atom of nitrogen and 3 atoms of hydrogen on the product side.

we can balance the hydrogens by placing a coefficient of 2 in front of ammonia and a coefficient of 3 in front of the hydrogen.

n2+3h2→2nh3

this gives us 6 hydrogen on each side and coincidentally the nitrogens now equal 2 on each side.