How many ammonia liters of ammonia gas are produced when 85 grams of liquid nitrogen completely react?
N2 + 3H2 = 2NH3
Assuming the process is at STP, 85gms N2 = 3.04 moles N2 => 2(3.04 moles NH3) => 2(3.04 moles)(22.4L/mol)NH3.
1500moles
Not! To much and in wrong units.
To calculate the amount of ammonia gas produced, we need to use the given balanced equation and the molar ratios between the reactants and products.
Step 1: Calculate the number of moles of liquid nitrogen:
To do this, we need to know the molar mass of nitrogen (N2). The molar mass of N2 is approximately 28 grams/mol.
Given:
Mass of liquid nitrogen (N2) = 85 grams
Molar mass of N2 = 28 g/mol
Number of moles of N2 = Mass / Molar mass
Number of moles of N2 = 85 g / 28 g/mol
Number of moles of N2 = 3.04 mol (rounded to two decimal places)
Step 2: Use the balanced equation to determine the molar ratio between N2 and NH3:
According to the balanced equation, 1 mole of N2 reacts to produce 2 moles of NH3.
Therefore, using the molar ratio:
Number of moles of NH3 = Number of moles of N2 × (2 moles of NH3 / 1 mole of N2)
Number of moles of NH3 = 3.04 mol × (2 mol / 1 mol)
Number of moles of NH3 = 6.08 mol (rounded to two decimal places)
Step 3: Convert moles of NH3 to volume in liters:
To do this, 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 ideal gas constant, and T is the temperature.
Since the volume and pressure are not given in the question, we assume that the reaction takes place at standard temperature and pressure (STP):
Temperature (T) = 273.15 K
Pressure (P) = 1 atm
At STP, 1 mole of any gas occupies 22.4 liters of volume.
Number of liters of NH3 = Number of moles of NH3 × (22.4 L / 1 mol)
Number of liters of NH3 = 6.08 mol × (22.4 L / 1 mol)
Number of liters of NH3 = 136.19 L (rounded to two decimal places)
Therefore, 85 grams of liquid nitrogen completely reacting produces approximately 136.19 liters of ammonia gas.