Answer:
0.116 moles of ammonia can be produced from the reaction of 4.0 liters of hydrogen at 50.0°C and 1.2atm of pressure with excess nitrogen.
Step-by-step explanation:
The balanced chemical equation for the reaction of hydrogen and nitrogen to form ammonia is:
N2(g) + 3H2(g) → 2NH3(g)
To determine how many moles of ammonia can be produced from the reaction of 4.0 liters of hydrogen at 50.0°C and 1.2atm of pressure with excess nitrogen, we need to use the ideal gas law equation:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
First, we need to convert the volume of hydrogen gas to moles using the ideal gas law equation:
n = PV/RT
where P is the pressure in atm, V is the volume in liters, R is the gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
n = (1.2 atm)(4.0 L)/(0.0821 L·atm/mol·K)(50.0°C + 273) = 0.174 mol H2
Since there is excess nitrogen, all of the hydrogen will react to form ammonia. Using the mole ratio between NH3 and H2 from the balanced chemical equation:
2 mol NH3 / 3 mol H2
we can calculate how many moles of NH3 will be produced:
n(NH3) = (0.174 mol H2) × (2 mol NH3 / 3 mol H2) = 0.116 mol NH3
Therefore, 0.116 moles of ammonia can be produced from the reaction of 4.0 liters of hydrogen at 50.0°C and 1.2atm of pressure with excess nitrogen.