In the decomposition of 2.5 moles of Chromium Hydroxide how many moles of water are produced?

Please be VERY descriptive on how to do this. I've been out of school a very long time and am expected to take a test on it tomorrow.

Here is an example of a stoichiometry problem.

http://www.jiskha.com/science/chemistry/stoichiometry.html

To determine the number of moles of water produced in the decomposition of 2.5 moles of Chromium Hydroxide (Cr(OH)3), we first need to understand the balanced chemical equation for the reaction.

The balanced equation for the decomposition of Chromium Hydroxide is:

Cr(OH)3 -> CrO3 + H2O

This equation shows that one mole of Chromium Hydroxide decomposes to produce one mole of Chromium Trioxide (CrO3) and one mole of water (H2O).

Now, since we know that 2.5 moles of Chromium Hydroxide are given, we can use the stoichiometry of the reaction to find the number of moles of water produced.

From the balanced equation, we can see that the molar ratio between Chromium Hydroxide and water is 1:1. This means that for every mole of Chromium Hydroxide decomposed, one mole of water is produced.

To calculate the number of moles of water produced, we simply use the given 2.5 moles of Chromium Hydroxide and multiply it by the molar ratio of water to Chromium Hydroxide, which is 1:

Number of moles of water = 2.5 moles of Chromium Hydroxide × (1 mole of water / 1 mole of Chromium Hydroxide)

Number of moles of water = 2.5 moles of Chromium Hydroxide

Therefore, in the decomposition of 2.5 moles of Chromium Hydroxide, 2.5 moles of water are produced.

Now you have the step-by-step explanation of how to solve this problem. Good luck with your test!