Question

write a balanced chemical equation based on the following description: solid cesium reacts with solid cesium nitrite to produce solid cesium oxide and nitrogen gas. 10 cs(s) + 2 csno₂(s) → 6 cs₂o(s) + n₂(g)

Explanation:

Step1: Check the number of Cs atoms

On the left side: \(10 + 2=12\) Cs atoms. On the right side: \(6\times2 = 12\) Cs atoms.

Step2: Check the number of N atoms

On the left side: \(2\) N atoms. On the right side: \(2\) N atoms.

Step3: Check the number of O atoms

On the left side: \(2\times2=4\) O atoms. On the right side: \(6\times1 = 6\) O atoms. This is incorrect. Let's re - balance.

Let the balanced equation be \(x\ Cs(s)+y\ CsNO_2(s)\to z\ Cs_2O(s)+w\ N_2(g)\)

For Cs: \(x + y=2z\)

For N: \(y = 2w\)

For O: \(2y=z\)

Let \(w = 1\), then \(y = 2\). If \(y = 2\), then from \(2y=z\), \(z = 4\). From \(x + y=2z\), \(x+2 = 8\), so \(x = 6\)

The balanced equation is \(6Cs(s)+2CsNO_2(s)\to4Cs_2O(s)+N_2(g)\)

Answer:

\(6Cs(s)+2CsNO_2(s)\to4Cs_2O(s)+N_2(g)\)