Calculate volume of ammonia gas produced at STP when 140g of nitrogen gas is reacted with 30g of hydrogen gas.
224 L
To calculate the volume of ammonia gas produced at STP (Standard Temperature and Pressure), we need to use the concept of stoichiometry and the Ideal Gas Law.
Here are the steps to follow:
1. Convert the given masses of nitrogen gas (N₂) and hydrogen gas (H₂) to moles. To do this, divide the given masses by their respective molar masses.
- The molar mass of N₂ is 28 g/mol.
- The molar mass of H₂ is 2 g/mol.
So, the number of moles of nitrogen gas (N₂) can be calculated as:
moles of N₂ = mass of N₂ / molar mass of N₂
= 140 g / 28 g/mol
= 5 moles
And the number of moles of hydrogen gas (H₂) can be calculated as:
moles of H₂ = mass of H₂ / molar mass of H₂
= 30 g / 2 g/mol
= 15 moles
2. Set up and balance the chemical equation for the reaction between nitrogen gas and hydrogen gas to form ammonia gas:
N₂ + 3H₂ → 2NH₃
3. Determine the stoichiometric ratio between nitrogen gas (N₂) and ammonia gas (NH₃) from the balanced chemical equation. In this case, according to the balanced equation, 1 mole of N₂ reacts to produce 2 moles of NH₃.
4. Since the stoichiometric ratio is given in moles, we can directly convert the number of moles of nitrogen gas to moles of ammonia gas using the stoichiometric ratio:
moles of NH₃ = moles of N₂ * (2 moles of NH₃ / 1 mole of N₂)
= 5 moles * (2 moles / 1 mole)
= 10 moles
5. Apply the Ideal Gas Law to calculate the volume of ammonia gas. The Ideal Gas Law equation is:
PV = nRT
At STP, the pressure (P) is 1 atm, the temperature (T) is 0°C or 273 K, and the ideal gas constant (R) is 0.0821 L•atm/(mol•K).
Plugging these values into the equation, we have:
V = (n * R * T) / P
= (10 moles * 0.0821 L•atm/(mol•K) * 273 K) / 1 atm
= 224.3 liters
Therefore, the volume of ammonia gas produced at STP when 140g of nitrogen gas reacts with 30g of hydrogen gas is 224.3 liters.