Question

In which of the following chemical equations, the abbreviations represent the correct states of the reactants and products involved at reaction temperature? (a) 2H2 (l) + O2 (l) → 2H2O(g) (b) 2H2 (g) + O2 (l) → 2H2O(l) (c) 2H2 (g) + O2 (g) → 2H2O(l) (d) 2H2 (g) + O2 (g) → 2H2O(g)

Answer 1

Answer:

option c..2H2(g)+O2(g)⟶2H2O(l)

Explanation:

2H2(g)+O2(g)⟶2H2O(l) is the correction reaction as during formation of water both hydrogen and oxygen are in gaseous form and produces water in liquid form.

Answer 2

The correct state of reactants and products is represented by $2H_2(g)+O_2(g)\rightarrow 2H_2O(l)$.

• The above reaction represents the preparation of water from hydrogen and oxygen gas.
• In this reaction, two moles of hydrogen in the gaseous state react with one mole of oxygen in the gaseous state to produce two moles of water in the liquid state.
• Hence the balanced reaction is written as follows-
• $2H_2(g)+O_2(g)\rightarrow 2H_2O(l)$.
• Hence the correct option is c.