3)What mass of propane could burn in 480 g of oxygen? C_(3)H_(8)+5O_(2)arrow 3CO_(2)+4H_(2)O

## Step1:The balanced chemical equation is given as . From this equation, we can see that 1 mole of propane ( ) reacts with 5 moles of oxygen ( ).## Step2:First, we need to find the molar mass of propane ( ) and oxygen ( ). The molar mass of propane is \( (3*12) + (8*1) = 44 \mathrm{~g/mol} \) and the molar mass of oxygen is \( (16*2) = 32 \mathrm{~g/mol} \).## Step3:Next, we calculate the number of moles of oxygen present by dividing the given mass of oxygen by its molar mass. Hence, the number of moles of oxygen is .## Step4:According to the stoichiometric coefficients in the balanced chemical equation, propane and oxygen react in a 1:5 molar ratio. Therefore, the moles of propane required is , i.e., .## Step5:Finally, the required mass of propane is calculated by multiplying the result in step 4 by the molar mass of propane. Hence, the mass of propane is .