Question

If you put 1.50 moles of N2 and 4.00 moles of O2 gas in a 45.0 L container at a temperature of 45°C, what is the total pressure of the system?

atm (use 3 sig figs)

Answer 1



Step-by-step explanation:

To solve this problem, we can use the ideal gas law:

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 in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin:

T = 273.15 + 45 = 318.15 K

Next, we can calculate the total number of moles of gas:

n = 1.50 moles N2 + 4.00 moles O2 = 5.50 moles

Now, we can rearrange the ideal gas law to solve for the pressure:

P = nRT/V

P = (5.50 mol)(0.0821 L·atm/mol·K)(318.15 K)/(45.0 L)

P = 2.03 atm

Therefore, the total pressure of the system is 2.03 atm, rounded to three significant figures.