Question

$H_2\left(g\right)+V_2{O}_5\left(s\right)🡪V_2{O}_3\left(s\right)+H_{2}O\left(l\right)$

Let the coefficients for the given reaction be as follows:

${\mathrm{wH}}_2\left(g\right)+{\mathrm{xV}}_2{O}_5\left(s\right)🡪{\mathrm{yV}}_2{O}_3\left(s\right)+{\mathrm{zH}}_{2}O\left(l\right)$

What will be the values of w, x, y and z when the reaction is balanced?

Answer 1

The balanced chemical equation is:

$4H_2\left(g\right)+2V_2{O}_5\left(s\right)🡪2V_2{O}_3\left(s\right)+4H_{2}O\left(l\right)$
Equating the number of atoms for each element on the two sides of the equation, we get:
w = z, x = y and 5x = 3y + z.
Where, w and z = number of H atoms, x and y = number of V atoms and number of O atoms are expressed as 5x = 3y + z.

The values of coefficients are such as:

w=4, x=2, y=2, and z=4.