Hi, I'm having diffuculty with this problem:
Given the equation:
CaH2(s) + 2H20(l) ---> 2H2(g) + Ca(OH)2(aq)
How many grams of CaH2 are needed to produce 14.00L of gas at 35 degrees celsius and 1.00 atm?

I used the following equation to get the moles n=(PV)/(RT) and then converted from moles of CaH2 to grams and got 23.3g of CaH2.

Is this answer correct or is it 11.7, because of 2 moles of H2?

If anyone could help me answer this question it would be greatly appreaciated.

First off you need to balance the original equation. Once you have done that, let me know. If it is already balanced let me know too.

I already know whether it is, but since this looks like homework, I will let you do the hard part.

LOL