Question

28.0 g of N2 gas was found to occupy a volume of 8.44 L at a pressure of 320 kPa what is the temperature of the gas

Answer 1

[AI-generated answer — Bot GPT 3.5]

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

PV = nRT

Where:
P = pressure in atmospheres (1 atm = 101.3 kPa)
V = volume in liters
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature in Kelvin

First, we need to convert the pressure from kPa to atm:
320 kPa / 101.3 kPa/atm = 3.16 atm

Now we can rearrange the formula to solve for T:
T = (P * V) / (n * R)

Given that the mass of N2 gas is 28.0 g, we can convert this to moles by dividing by the molar mass of N2 (28.02 g/mol):
n = 28.0 g / 28.02 g/mol = 1.0 mol

Plugging in the values, we get:
T = (3.16 atm * 8.44 L) / (1.0 mol * 0.0821 L.atm/mol.K)
T = 27.62 K

Therefore, the temperature of the gas is 27.62 K.