Question

Given that 4.75 moles of carbon monoxide gas are present in a container of volume 12.50 L, what is the pressure of the gas (in atm) if the temperature is 77°C?

Answer 1

We can use the Ideal Gas Law to solve this problem, which relates the pressure (P), volume (V), number of moles (n), and temperature (T) of a gas:

PV = nRT

where R is the ideal gas constant, which has a value of 0.0821 L·atm/mol·K.

First, we need to convert the temperature from Celsius to Kelvin by adding 273.15:

T = 77°C + 273.15 = 350.15 K

Next, we can plug in the given values and solve for the pressure:

P = nRT/V

P = (4.75 mol)(0.0821 L·atm/mol·K)(350.15 K)/(12.50 L)

P = 11.8 atm

Therefore, the pressure of the carbon monoxide gas is 11.8 atm when the volume is 12.50 L and the temperature is 77°C.