Oxygen gas reacts with hydrogen to produce water. The reaction is represented by the equation :
$O_{2} (g) + H_{2} (g) \to H_{2} O (g)$ .
The above reaction is an example of
(a)Oxidation of hydrogen
(b)Reduction of oxygen
(c)Reduction of hydrogen
(d)Redox reaction
(b), (c) and (d)
(a),(c) and (d)
(a), (b) and (c)
(a),(b) and (d)

Question

Oxygen gas reacts with hydrogen to produce water. The reaction is represented by the equation :
$O_{2} (g) + H_{2} (g) \to H_{2} O (g)$ .
The above reaction is an example of
(a)Oxidation of hydrogen
(b)Reduction of oxygen
(c)Reduction of hydrogen
(d)Redox reaction
(b), (c) and (d)
(a),(c) and (d)
(a), (b) and (c)
(a),(b) and (d)

Toppr Admin · Accepted Answer

The correct option is D -a-b- and -d-O2-H2-x2192-H2O-g-O-S-of-xA0-O2become-x2192-zeroto-x2212-2-x2235- it will be reduced and oxidation state of H2 becomes zero to -1 it will be oxidised-x2234- reaction will be redox

The correct option is D (a),(b) and (d)O2+H2→H2O(g)O.S.of O2become→zeroto−2∵ it will be reduced and oxidation state of H2 becomes zero to +1 it will be oxidised.∴ reaction will be redox

The correct option is D (a),(b) and (d)
$O_{2} + H_{2} \to H_{2} O_{(g)}$
O.S.of $O_{2} b e c o m e \to z e r o t o - 2$
$∵$ it will be reduced and oxidation state of $H_{2}$ becomes zero to $+ 1$ it will be oxidised.
$∴$ reaction will be redox