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1) That looks right. 2) Step 1: Moles=Mass/Mr, so it's 144/72= 2mol. Step 2: Stoichiometry means the ratio of oxygen to pentane is 1:8 so moles of oxygen is moles of pentane times 8. 2*8=16mol of oxygen. Step 3: 16= 9.6*10^24. 3) The ratio of oxygen to carbon in CO2 is 1:2. so it's 192/3 = 64.
Use Avogadroâs law to determine the number of moles of butane gas. Assume that butane is an ideal gas and that one mole has a volume of 22.4 L at STP. V 1 /n 1 = V 2 /n 2 0.0896 L/n = 22.4 L/1 mole n = 0.0040 moles 12. Experimental molar mass (g/mole) of butane: 0.23 g/0.0040 moles = 58 g/mole 13.The molecular formula of butane is C 4 H 10.Calculate its molar mass.se the combined gas law to determine the volume (in L) of butane at STP.11. Use Avogadroâs law to determine the number of moles of butane gas. Assume that butane is an ideal gas and that one mole has a volume of 22.4 L at STP.12. Experimental molar mass (g/mole) of butane13.