Question
Determine the pressure (in atm) of 42.3 g N2 at 36.4 C in 6.93 L. Be sure your answer has the correct number of significant figures.
Note: Reference the Fundamental constants table for additional information.
Note: Reference the Fundamental constants table for additional information.
Answers
GPT 3.5
1. Calculate the number of moles of N2 using the formula:
moles = mass / molar mass
molar mass of N2 = 28.02 g/mol
moles = 42.3 g / 28.02 g/mol
moles = 1.51 mol
2. Use the ideal gas law equation to calculate the pressure:
PV = nRT
where:
P = pressure
V = volume = 6.93 L
n = moles = 1.51 mol
R = gas constant = 0.08206 L.atm/mol.K
T = temperature in Kelvin = 36.4 + 273.15 = 309.55 K
Plugging in the values:
P * 6.93 = 1.51 * 0.08206 * 309.55
P = (1.51 * 0.08206 * 309.55) / 6.93
P = 2.8 atm
Therefore, the pressure of 42.3 g N2 at 36.4 C in 6.93 L is 2.8 atm. This answer has two significant figures.
moles = mass / molar mass
molar mass of N2 = 28.02 g/mol
moles = 42.3 g / 28.02 g/mol
moles = 1.51 mol
2. Use the ideal gas law equation to calculate the pressure:
PV = nRT
where:
P = pressure
V = volume = 6.93 L
n = moles = 1.51 mol
R = gas constant = 0.08206 L.atm/mol.K
T = temperature in Kelvin = 36.4 + 273.15 = 309.55 K
Plugging in the values:
P * 6.93 = 1.51 * 0.08206 * 309.55
P = (1.51 * 0.08206 * 309.55) / 6.93
P = 2.8 atm
Therefore, the pressure of 42.3 g N2 at 36.4 C in 6.93 L is 2.8 atm. This answer has two significant figures.