Question

12.2 g of N₂ gas at 1132 torr and 91°C has a volume of

Answer 1

Answer:

8.73 L

Explanation:

First, you need to convert grams to moles using the molar mass.

Molar Mass (N₂): 2(14.009 g/mol)

Molar Mass (N₂): 28.018 g/mol

12.2 grams N₂               1 mole
----------------------  x  ------------------------  =  0.435 moles N₂
                                 28.018 grams

To find the volume, you need to use the Ideal Gas Law:

PV = nRT

In this equation,

-----> P = pressure (torr)

-----> V = volume (L)

-----> n = moles

-----> R = Ideal Gas constant (62.36 torr*L/mol*K)

-----> T = temperature (K)

After converting the temperature from Celsius to Kelvin, you can plug the given values into the equation.

P = 1132 torr                                   R = 62.36 torr*L/mol*K

V = ? L                                            T = 91 °C + 273.15 = 364.15 K

n = 0.435 moles

PV = nRT

(1132 torr)V = (0.435 moles)(62.36 torr*L/mol*K)(364.15 K)

(1132 torr)V = 9888.015

V = 8.73 L