Physics Homework Solutions
#3217
Calculating moles and molecular mass in a gas law problem.
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?
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