# Producing methane, reactants and products [closed]

How do I balance this reaction when producing methane using the reactants:

$$\ce{CH3COONa(s) + NaOH(s) + Ca(OH)2 -> ?}$$

The products are partly

$\ce{CH4(g) + Na2CO3(s)}$

What else is missing in the products? Furthermore, how do I balance this?

## closed as off-topic by M.A.R. ಠ_ಠ, Wildcat, ron, airhuff, paracetamolMay 6 '17 at 16:45

This question appears to be off-topic. The users who voted to close gave this specific reason:

If this question can be reworded to fit the rules in the help center, please edit the question.

• This is a homework question. We have a policy which states that ‎you should show your thoughts and/or efforts into solving the problem. It'll make us certain that ‎we aren't doing your homework for you. Otherwise, this question may get closed.‎ Please edit in your full reasoning or thoughts on this. – M.A.R. ಠ_ಠ May 6 '17 at 12:02

$$\ce{2CH3COONa(s) + 2NaOH(s) + Ca(OH)2(s) <=> 2CH4(g) + Na2CO3(s) + CaCO3(s) + H2O}$$
There are $2\times 3 + 2\times 1 + 2\,$ hydrogen atoms in left side, and there are $2\times 4 + 2$ $\ce{H}$ in the right side. So both sides give $10$ hydrogen atoms.