Question

For the reaction below, calculate how many moles of the product form when 0.026 mol of O2 completely reacts. Assume that there is more than enough of the other reactant.

2Ca(s)+O2(g)→2CaO(s)

Express your answer using two significant figures.

Answer 1

In a balanced chemical reaction the numbers signify the mole numbers used in the reaction.

So from the above reaction we can easily say that from one mole oxygen two moles of CaO is produced. That means if we start from 1 mole of oxygen and after it fully reacts we will end up with 2 moles of product.

Here we have started this reaction with 0.026 moles of O2. Thus after complete reaction we will have 2*0.026=0.052 moles of product.

To complete the reaction the other reactant which is Ca here must be sufficient. So the condition of excess Ca is given.