Hydrogen and oxygen react to produce water, according to the reaction

2 H2 (g) + O2 (g) → 2 H2O (l).

If 3 moles of hydrogen react with 2 moles of oxygen and the yield in the reaction is 80%, how many moles of water are obtained?

3 mol

Explanation:

Given data:

Moles of hydrogen = 3 mol

Moles of oxygen = 2 mol

Yield of reaction = 80%

Moles of water produced = ?

Solution:

Chemical equation:

2H₂ + O₂  →  2H₂O

Now we will compare the moles of water with both reactants.

                       H₂           :         H₂O

                        2            :            2

                          3          :             3

                          O₂        :           H₂O

                           1          :              2

                           2          :         2×2 =   4

Hydrogen produced less number of moles of water so it will limiting reactant.

So number of moles of water produced are = 3 mol

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.