Question

Consider the combustion of h2(g) 2h2(g)+o2(g)→2h2o(g). If hydrogen is burning at the rate of 0.49 mol/s, what is the rate of consumption of oxygen

Answer 1

Answer : The rate of consumption of oxygen = 0.245 mol/s

Solution :  Given,

                 Rate at which Hydrogen burns = 0.49 mol/s

                 The Reaction is,

                       $2H_{2}(g)+O_{2}(g)\rightarrow 2H_{2}O(l)$

    In this reaction,  2 moles of hydrogen react with the 1 mole of oxygen.

    The rate at which oxygen burns is equal to the half of rate at which hydrogen burns.

     Rate at which Oxygen burns = $\frac{1}{2}$ × 0.49 mol/s

                                                      = 0.245 mol/s