Question

N2 + 3H2 - ...> 2NH3

How many liters of NHs will be produced at a temperature of 208.00 degrees celsius and 4.50 torr pressure to consume 26.00 moles of N2?
Round to two decimal places.

Answer 1

To solve this problem, we need to use the ideal gas law to find the volume of NH3 produced. The ideal gas law is 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 find the volume of N2 consumed:

PV = nRT

V = nRT/P

V = (26.00 mol)(0.08206 L·atm/mol·K)(481.15 K)/(4.50 torr/760 torr/atm)

V = 91.9 L

According to the balanced chemical equation, 2 moles of NH3 are produced for every 1 mole of N2 consumed. Therefore, the number of moles of NH3 produced is:

n(NH3) = 2 x n(N2) = 2 x 26.00 mol = 52.00 mol

Next, we can use the ideal gas law to find the volume of NH3 produced:

PV = nRT

V = nRT/P

V = (52.00 mol)(0.08206 L·atm/mol·K)(481.15 K)/(4.50 torr/760 torr/atm)

V = 183.7 L

Therefore, the volume of NH3 produced is 183.7 liters, rounded to two decimal places.