Question
You have 229 mL of chlorine trifluoride gas at 735 mmHg and
30
°
C. What is the mass (in g) of the sample?
g
30
°
C. What is the mass (in g) of the sample?
g
Answers
GPT 3.5
To determine the mass of the sample, we need to use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure in atm (convert mmHg to atm by dividing by 760: 735 mmHg / 760 = 0.966 atm)
V = volume in liters (convert mL to L by dividing by 1000: 229 mL / 1000 = 0.229 L)
n = number of moles of gas
R = ideal gas constant = 0.0821 L·atm/(mol·K)
T = temperature in Kelvin (convert Celsius to Kelvin: 30 + 273 = 303 K)
Rearranging the equation to solve for n:
n = (PV)/(RT)
n = (0.966 atm * 0.229 L) / (0.0821 L·atm/(mol·K) * 303 K)
n = 0.3004 mol
Since the molar mass of chlorine trifluoride (ClF3) is approximately 92.45 g/mol, we can calculate the mass of the sample:
mass = n * molar mass
mass = 0.3004 mol * 92.45 g/mol
mass ≈ 27.64 g
Therefore, the mass of the sample is approximately 27.64 g.
PV = nRT
Where:
P = pressure in atm (convert mmHg to atm by dividing by 760: 735 mmHg / 760 = 0.966 atm)
V = volume in liters (convert mL to L by dividing by 1000: 229 mL / 1000 = 0.229 L)
n = number of moles of gas
R = ideal gas constant = 0.0821 L·atm/(mol·K)
T = temperature in Kelvin (convert Celsius to Kelvin: 30 + 273 = 303 K)
Rearranging the equation to solve for n:
n = (PV)/(RT)
n = (0.966 atm * 0.229 L) / (0.0821 L·atm/(mol·K) * 303 K)
n = 0.3004 mol
Since the molar mass of chlorine trifluoride (ClF3) is approximately 92.45 g/mol, we can calculate the mass of the sample:
mass = n * molar mass
mass = 0.3004 mol * 92.45 g/mol
mass ≈ 27.64 g
Therefore, the mass of the sample is approximately 27.64 g.