Explore BrainMass

Explore BrainMass

    Calculating moles and molecular mass

    This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here!

    A steel bottle of 4.00 liters, initially evacuated, is filled with 4.00 grams of a pure gas. The bottle has an absolute pressure of 1.5375 Standard Atmospheres when the temperature is 300 Kelvin. R=0.0820 liter atm/mole K.

    1) How many moles of gas does the bottle contain?

    2) What's the molecular weight (in grams) of the mass?

    3) If the gas is a hydrocarbon compound known to be a member of the paraffin series, CnH2n+2, what is the chemical formula of the compound?

    © BrainMass Inc. brainmass.com March 4, 2021, 5:37 pm ad1c9bdddf
    https://brainmass.com/physics/ideal-gas-law/calculating-moles-molecular-mass-3217

    Solution Preview

    1) To solve for the number of moles of gas, we can use the ideal gas law which says that P V = n R T. This can be rewritten as n = P V / (R T) to give the number of moles of gas. Since the volume (4 liters), pressure (1.5375 atm) and temperature (300K) are known you can calculate the ...

    Solution Summary

    The expert calculates the moles and molecular mass achieved. The molecular weight of the mass is determined.

    $2.49

    ADVERTISEMENT