A sample of gas has a mass of 0.580g . Its volume is 119mL at a temperature of 80∘C and a pressure of 743mmHg .
Find the molar mass of the gas.
I think I got a step wrong in the problem, please help?
so, what steps did you follow? If you want help with your error, show your work...
To find the molar mass of the gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure in atm
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 given values to the appropriate units:
0.580g = 0.580/1000 = 0.000580 kg (mass conversion to kg)
119mL = 119/1000 = 0.119 L (volume conversion to L)
80˚C = 80 + 273.15 = 353.15 K (temperature conversion to K)
743mmHg = 743/760 = 0.976 atm (pressure conversion to atm)
Now, rearranging the ideal gas law equation to solve for the number of moles (n):
n = PV/RT
Substituting the given values:
n = (0.976 atm) * (0.119 L) / (0.0821 L.atm/mol.K * 353.15 K)
Simplifying the calculation:
n = 0.0137 mol
Finally, to find the molar mass (M) of the gas, we can use the equation:
M = mass / number of moles
Substituting the given values:
M = 0.000580 kg / 0.0137 mol
Calculating:
M ≈ 42.34 g/mol
Therefore, the molar mass of the gas is approximately 42.34 g/mol.