Question

If a 7.00 gram sample of diatomic nitrogen at 10. °C occupies 2.50 L, what is the pressure of the sample?

Answer 1

To calculate the pressure of the sample using the ideal gas law, you can use the formula:

PV=nRT

Where:

P :is the pressure,

V :is the volume,

n :is the number of moles of the gas,

R :is the ideal gas constant,

T :is the temperature in Kelvin.

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

T(K)=T(°C)+273.15

T=10 °C +273.15=283.15 K

Calculate the moles of N2 :

n= mass/molar mass=7.00g/28g/mol=0.25mol

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

P=nRT/V

P=(7.00g/28g/mol ) • (0.821L atm/mol K) • (283.15K) = 2.16 atm

Answer:
The pressure of the sample is approximately 2.16 atm.