Question

Which one of the following statements about the following reaction is false? CH2(g) + 20%(9) CO2(g) + 2H2O(g) (a) Every methane molecule that reacts produces two water molecules. (b) If 32.0 g of oxygen reacts with excess methane, the maximum amount of carbon dioxide produced will be 22.0 g. (c) If 11.2 liters of methane react with an excess of oxygen, the volume of carbon dioxide produced at STP is (44/16)(11.2) liters. (d) If 16.0 g of methane react with 64.0 g of oxygen, the combined masses of the products will be 80.0 g. (e) If 22.4 liters of methane at STP react with 64.0 g of oxygen, 22.4 liters of carbon dioxide at STP can be produced.

Answer 1

From the balanced equation we can clearly see 1 molecule of methane produces 2 molecules of H2O. So a is true

32 grams of O2 means 1 mole of O2 . So from the equation we can see 1 mole of O2 will produce 1/2 mole of CO2 = 1/2 ×44=22grams. So b is also true

11.2 liters of methane implies 1/2 moles of methane as one mole of gas has a volume of 22.4 liters at STP. So 1/2 moles of methane will produce 1/2 moles of CO2 that is 11.2 liters of CO2 at STP

So statement c is false.