Question

When the equation shown below is balanced, what is the coefficient for Cs2O ? Cs + O2 → Cs2O (1 point) Responses 1 1 2 2 3 3 4

Answer 1

To balance the equation \( Cs + O_2 \rightarrow Cs_2O \), we need to ensure that the number of each type of atom on the reactant side equals the number on the product side.

The unbalanced equation shows:
- On the product side, Cs2O has 2 cesium (Cs) atoms and 1 oxygen (O) atom.
- On the reactant side, we start with Cs and \( O_2 \), which has 2 oxygen atoms.

To balance the equation:
1. We can start by putting a coefficient of 2 in front of Cs on the reactant side to have 2 Cs atoms:
\[
2 Cs + O_2 \rightarrow Cs_2O
\]

2. Now we check the balance:
- Reactants: 2 Cs, 2 O
- Products: 2 Cs, 1 O

3. To balance the oxygen, we can place a coefficient of 1/2 in front of \( O_2 \). However, since we cannot use fractions in our coefficients, we double everything:
\[
4 Cs + 2 O_2 \rightarrow 2 Cs_2O
\]

Now we have:
- Reactants: 4 Cs, 4 O
- Products: 4 Cs, 2 O (from 2 \( Cs_2O \))

Thus, the balanced equation is:
\[
4 Cs + O_2 \rightarrow 2 Cs_2O
\]

The coefficient for \( Cs_2O \) in the balanced equation is \( 2 \).

Therefore, the coefficient for \( Cs_2O \) is **2**.