[thelegace]

Hi, I am trying to figure out the problem, it seems simple to answer but Im not getting the right answer.

The reaction of calcium hydride and water produces calcium hydroxide and hydrogen as products.

How many moles of H_2(g) will be formed in the reaction between 0.50mol CaH_2(s) and 1.36mol  H_2O(l)? What is the answer in 2 significant figures?

Since the chemical reaction should be CaH_2(s) + 2H20(l) --> Ca(OH)_2(l) + 2H_2(g). The number of moles of water will produce the same amount of moles of hydrogen gas. So the answer in 2 sig figures would be 1.4mol but that answer doesn't seem to be right.

Thank You.

[LQ43]

Consider how much H2 will be produced from each reactant.