[manilal326]

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.

[J_9]

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