mass= 3.8721g
temperature= 102 degrees Celsius
volume= 156ml
atmospheric pressure= 755.0 mm Hg
calculate the molar mass using the ideal gas law
Use PV = nRT to solve for n = number of moles. Don't forget that T is in Kelvin.
Then n = grams/molar mass
You know n and grams, solve for molar mass.
so all the units i have to change is just for temperature and then leave the rest as they are
No. T is in Kelvin.
P is in atmospheres.
V is in L.
Use 0.08206 L*atm/mol*K for R.
To calculate the molar mass using the ideal gas law, you would need to rearrange the equation to solve for the molar mass.
The ideal gas law is expressed as: PV = nRT
Where:
P = pressure (in units of force/area)
V = volume (in units of length^3)
n = number of moles
R = ideal gas constant (8.314 J/mol·K)
T = temperature (in units of Kelvin)
To calculate the molar mass, you can rearrange the equation as follows:
n = PV / RT
Given values:
P = 755.0 mm Hg
V = 156 ml
R = 8.314 J/mol·K
T = 102 degrees Celsius = 375.15 Kelvin
Note that it's important to convert the temperature to Kelvin since the ideal gas law requires temperature in Kelvin.
Now, let's substitute the values into the equation:
n = (755.0 mm Hg) * (156 ml) / (8.314 J/mol·K * 375.15 K)
To convert the given pressure to the appropriate unit for the ideal gas law, we need to convert from mm Hg to atm. Since 1 atm = 760 mm Hg, we can calculate:
n = (755.0 mm Hg / 760 mm Hg/atm) * (156 ml) / (8.314 J/mol·K * 375.15 K)
Simplifying:
n = (0.9947 atm) * (156 ml) / (8.314 J/mol·K * 375.15 K)
The volume is given in milliliters (ml), which needs to be converted to liters (L) because the ideal gas constant (R) is in units of J/mol·K. There are 1000 ml in a liter, so we have:
n = (0.9947 atm) * (0.156 L) / (8.314 J/mol·K * 375.15 K)
Finally, let's calculate the molar mass:
molar mass = mass / number of moles
Given mass = 3.8721 g, and we have calculated the number of moles as:
n = (0.9947 atm) * (0.156 L) / (8.314 J/mol·K * 375.15 K)
molar mass = 3.8721 g / ((0.9947 atm) * (0.156 L) / (8.314 J/mol·K * 375.15 K))