How many moles of H2(g) will be formed in the reaction between 0.99 mol CaH2}(s) and 1.32 mol H2O(l)?

To determine the number of moles of H2(g) formed in the reaction, we need to use the balanced chemical equation for the reaction between CaH2 and H2O.

The balanced chemical equation is:

CaH2(s) + 2H2O(l) -> Ca(OH)2(aq) + 2H2(g)

From the equation, we can see that for every one mole of CaH2(s), two moles of H2(g) are formed.

Given that we have 0.99 moles of CaH2(s), we can calculate the number of moles of H2(g) as follows:

0.99 mol CaH2(s) x (2 mol H2(g) / 1 mol CaH2(s)) = 1.98 mol H2(g)

Therefore, 1.98 moles of H2(g) will be formed in the reaction between 0.99 mol of CaH2(s) and 1.32 mol of H2O(l).