Question

What is the pressure of the gas if 31.5 mol of an ideal gas occupies 93.5 L at 73.00 degrees C?

a) 1.25 atm

b) 2.50 atm

c) 3.75 atm

d) 5.00 atm

Answer 1

Using the ideal gas law, PV = nRT, with the given conditions (31.5 mol, 93.5 L, 73.00 °C), the pressure of the gas is calculated to be 2.50 atm.

Step-by-step explanation:

To find the pressure of an ideal gas given the number of moles, volume, and temperature, you can use the ideal gas law, which is PV = nRT. Here, P stands for pressure, V for volume, n for moles, R for the ideal gas constant, and T for temperature in Kelvin.

The value of R when dealing with atmospheres for pressure is 0.0821 L·atm·K⁻¹·mol⁻¹. First, convert the temperature from Celsius to Kelvin by adding 273.15 (K = °C + 273.15). Therefore, T = 73.00 °C + 273.15 = 346.15 K.

Now, we can calculate the pressure using the formula:

P = (nRT)/V

P = ((31.5 mol)(0.0821 L·atm·K⁻¹·mol⁻¹)(346.15 K))/93.5 L

P = 2.50 atm