If 2.33 L of propane at 24 degrees C and 67.2 kPa is completely burned in excess oxygen, how many moles..?

of carbon dioxide will be produced? please help me

If 2.33 L of propane at 24 degrees C and 67.2 kPa is completely burned in excess oxygen, how many moles..?
Let's write the balanced equation:





C3H8 + 10O2 --%26gt; 3CO2 + 4H2O





We'll use the ideal gas law so that we know how many moles of C3H8 (propane) are there. after knowing how many moles of C3H8, we can just convert to moles of CO2 (using the mole ratio, of course. Sweet and simple. :) )





Convert 24 C to Kelvin. Just add 273.





n = PV / RT


= (67.2)(2.33) / (8.314)(297)


= 0.0634 mol





BTW, since the unit of pressure is in kPa, we'll use the R (ideal gas constant value) of 8.314 L*kPa / mol* K





then, convert 0.0634 mol C3H8 to moles of CO2. Just use the mole ratio (get it from the coefficients of the balanced chemical equation) between C3H8 and CO2. The mole ratio is 1:3.





0.0634 mol C3H8 * 3 mol CO2 / 1 mol C3H8 = 0.190 mol CO2





:)

cvs