Question

What is the pressure of H2 gas if you have 0.412 moles of it at 289.15K in a 3.25L container?

a) 0.201 atm
b) 1.185 atm
c) 2.323 atm
d) 3.532 atm

Answer 1

Using the Ideal Gas Law and the provided values, the pressure of H2 gas was calculated to be 3.532 atm, as all the values were already in the correct units for the calculation.

Step-by-step explanation:

To find the pressure of H2 gas, we can use the Ideal Gas Law, which is PV = nRT. Here, P represents pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, we need to ensure that our given values are in the correct units: temperature in Kelvin and volume in liters. The container's volume is already given in liters (3.25 L), and the temperature in Kelvin is given as 289.15 K.

The ideal gas constant R in terms of atmospheres is 0.08206 L atm mol-1 K-1.

Now we can plug the values into the Ideal Gas Law and solve for P:

P = (nRT)/V = (0.412 moles)(0.08206 L atm mol-1 K-1)(289.15 K) / 3.25 L = 3.532 atm

Therefore, the pressure of H2 gas in the container is 3.532 atm.