Questions: Let's start by balancing the following chemical reaction fill in blank V(s) + fill in blank O2(g) → fill in blank V2 O5(s)

Solution Steps

The unbalanced chemical equation is given as:

\[ V(s) + \mathrm{O}_{2}(g) \rightarrow V_{2}O_{5}(s) \]

To balance the vanadium (V) atoms, we need to ensure that the number of V atoms on the reactant side equals the number on the product side. In the product \(V_{2}O_{5}\), there are 2 V atoms. Therefore, we need 2 V atoms on the reactant side:

\[ 2V(s) + \mathrm{O}_{2}(g) \rightarrow V_{2}O_{5}(s) \]

Next, we balance the oxygen (O) atoms. In the product \(V_{2}O_{5}\), there are 5 O atoms. Therefore, we need 5 O atoms on the reactant side. Since each \(O_{2}\) molecule contains 2 O atoms, we need \(\frac{5}{2}\) or 2.5 \(O_{2}\) molecules:

\[ 2V(s) + \frac{5}{2}\mathrm{O}_{2}(g) \rightarrow V_{2}O_{5}(s) \]

To eliminate the fraction, multiply the entire equation by 2:

\[ 4V(s) + 5\mathrm{O}_{2}(g) \rightarrow 2V_{2}O_{5}(s) \]

Final Answer