Consider the reaction represented by the following equation: C\(_2\)H\(_2\) + yH\(_2\) → C\(_2\)H\(_6\). The value of y in the reaction is
Answer Details
In the given reaction, C\(_2\)H\(_2\) and H\(_2\) react to form C\(_2\)H\(_6\). The molecular formula of C\(_2\)H\(_2\) is C\(_2\)H\(_2\) and that of H\(_2\) is H\(_2\). The molecular formula of C\(_2\)H\(_6\) is C\(_2\)H\(_6\). Therefore, we can write the balanced chemical equation as:
C\(_2\)H\(_2\) + 2H\(_2\) → C\(_2\)H\(_6\)
We can see that for every one mole of C\(_2\)H\(_2\) used in the reaction, two moles of H\(_2\) are required. Therefore, the value of y in the equation is 2. So, the correct option is (C) 2.