When electric current is supplied through an ionic hydride of fused state, then:
A. Hydrogen is obtained at anode
B. Hydrogen is obtained at cathode
C. No change
D. Hydride ion moves towards cathode
E. Hydride ion present in solution

Hint: A process in which electricity passes through the electrolyte and a chemical reaction occurs is termed electrolysis. In the electrolysis process, chemical energy is converted to electrical energy.

Complete Step by Step Solution:
Let's understand the electrochemical cell in detail. There are two electrodes namely cathode and anode that consist of an electrochemical cell. These electrodes are placed in a solution called electrolytes and two half cells are formed. When combined, these half cells lead to a cell's formation.

Now, come to the question. It is given that the supply of electric current through an ionic hydride takes place.
A metal ion dissociates in the following way:
\[{\rm{MH}}\rightleftharpoons {{\rm{M}}^ + } + {{\rm{H}}^ - }\]

At anode, oxidation of hydride ions occurs. The oxidation reaction liberates hydrogen gas at anode.
\[{\rm{2}}{{\rm{H}}^ - } \to {{\rm{H}}_{\rm{2}}} + 2{e^ - }\]

At cathode, cation of metal accepts electrons to form the metal.
\[{{\rm{M}}^ + } + {e^ - } \to {\rm{M}}\]

Therefore, the liberation of hydrogen occurs at the anode on passing an electric current through an ionic hydride.
Hence, option A is the right answer.

Note: It is to be noted that the process of losing electrons by atoms is termed oxidation and the process of electron gain by an ion is termed reduction. The anode is the electrode of an electrochemical cell where oxidation reaction occurs and at the cathode reduction reaction occurs.