A sample of krypton gas in a container of volume 1.90 L exerts a pressure of 0.553 atm at 21 Celsius. How many moles of gas are present?

A sample of 0.0435 mol of krypton in a 1.90 L container exerts a pressure of 0.553 atm at 21 °C.

We have a sample of krypton gas in a 1.90-L (V) container that exerts a pressure (P) of 0.553 atm at 21 °C (T). We can calculate the moles (n) of krypton using the ideal gas law.

It is an equation of state of an ideal gas that relates pressure, volume, moles of gas, and temperature. The mathematical expression is:

P × V = n × R × T

where R is the ideal gas constant (0.0821 atm.L/mol.K)

To apply this law, first, we must convert 21 °C to Kelvin using the following expression.

K = °C + 273.15 = 21°C + 273.15 = 294 K

The moles of krypton are:

P × V = n × R × T

n = P × V/R × T

n = 0.553 atm × 1.90 L/(0.0821 atm.L/mol.K) × 294 K = 0.0435 mol

A sample of 0.0435 mol of krypton in a 1.90 L container exerts a pressure of 0.553 atm at 21 °C.

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0.044 mole

Explanation:

Data obtained from the question include:

V (volume) = 1.90 L

P (pressure) = 0.553 atm

T (temperature) = 21°C = 21 + 273 = 294K

R (gas constant) = 0.082atm.L/Kmol

n (number of mole of krypton) =?

Using the ideal gas equation PV = nRT, the number of mole of krypton can obtained as illustrated below:

PV = nRT

n = PV /RT

n = (0.553 x 1.9)/(0.082x294)

n = 0.044 mole

Therefore, 0.044 mole of krypton is present in the container.

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .