What is needed to calculate the mass of ammonia gas produced from 2.0 L of nitrogen gas in excess hydrogen gas in the reaction below?

N2(g) + 3H2(g) ® 2NH3(g)

You can use a shortcut method when everything is in the gaseous form.

N2 + 3H2 ==> 2NH3.

2.0 L N2 x (2 moles NH3/1 mole N2) = 2 x (2/1) = 4 L NH3 produced.

To calculate the mass of ammonia gas produced from 2.0 L of nitrogen gas, you need to use the stoichiometry of the balanced chemical equation. The coefficients in the balanced equation represent the ratio of moles between the reactants and products.

In this case, the balanced equation is:

N2(g) + 3H2(g) → 2NH3(g)

Based on the balanced equation, you can see that:

- For every 1 mole of N2, 2 moles of NH3 are produced.
- For every 3 moles of H2, 2 moles of NH3 are produced.

Since you are given the volume of N2 gas (2.0 L), you need to convert this volume to moles using the ideal gas law. The ideal gas law equation is:

PV = nRT

Where:
P = Pressure of the gas
V = Volume of the gas
n = Number of moles of gas
R = Ideal gas constant (0.0821 L·atm/mol·K)
T = Temperature of the gas (in Kelvin)

Assuming the conditions are at standard temperature and pressure (STP), which is 0 °C (273 K) and 1 atm, you can use the equation to calculate the moles of N2 gas.

Next, you need to determine the limiting reactant. Since excess hydrogen gas is provided, the limiting reactant will be the one that produces the least amount of ammonia. The stoichiometry of the equation tells us that 1 mole of N2 produces 2 moles of NH3.

Once you find the moles of N2, you can use the stoichiometry of the equation to calculate the moles of NH3 produced. Multiply the moles of N2 by the stoichiometric ratio (2 moles NH3 / 1 mole N2) to find the moles of NH3 produced.

Finally, to determine the mass of NH3 produced, you need to use the molar mass of NH3, which is 17.03 g/mol. Calculate the mass by multiplying the moles of NH3 produced by the molar mass.

By following these steps, you will be able to calculate the mass of ammonia gas produced from 2.0 L of nitrogen gas in excess hydrogen gas.