Solve this problem using the appropriate law. (Remember that) What is the pressure of 1.9 mols of nitrogen gas in a 9.45 L tank and at a temperature of 228 K?

PV=nRT

You are funding pressure and you have V = 9.45L, n = 1.9 moles, R = gas constant, and T = 228 K

P (9.45L) = (1.9moles) (0.0821) (228K)

Find P

Multiply

9.45P = 35.57

Divide

P = 3.76 L of N

Answer should be 3.76 liters of nitrogen

P = 3.7635 atm

Explanation:

We can use any law that involves pressure. However, as we are talking here of a gas, we better use the ideal gas equation, which is shorter and easier to use.

The ideal gas equation is:

PV = nRT

And solving for P:

P = nRT/V

Where:

P: Pressure in atm

n: moles of the gas

R: gas constant which is 0.0821 L atm / mol K

V: Volume of the gas or container

T: Temperature of the reaction or container.

In this case, we have all the data, so we just replace the given data in the above expression to calculate pressure:

P = 1.9 * 0.0821 * 228 / 9.45

P = 35.56572 / 9.45

P = 3.7635 atm

This is the pressure of nitrogen gas.