Question

Upon balancing the equation below, how many moles of sodium cyanide are needed to react completely with 3.6 moles of sulfuric acid?

H2SO4 + NaCN yields HCN + Na2SO4

1.2 mol NaCN

1.8 mol NaCN

3.6 mol NaCN

7.2 mol NaCN

Answer 1

Just looking at H and CN, how much CN do you need in the reaction to completely react with all the H?

Answer 2

um, 3.6?

Answer 3

Um. A mole has the some number of molecules no matter what the substance correct?

So how many atoms of H are there in 3.6 moles of H"2"SO4?

And so how many atoms of CN do you need to react with the H to yield HCN?

So how molecules of NaCN do you need to supply that many atoms of CN?

Answer 4

I should say how many moles of NaCN do you need to supply that many atoms of CN.

Answer 5

We could write formulas if you wish and solve them. I can help you with that if you would prefer.

Answer 6

Hm.

H2SO4 + NaCN -> HCN + Na2SO4

There are 2 hydrogens on one side and only one on the yield side.
Same for Na, one on the reactants side and 2 on the yield side.

Balance the equation. Then the factors will reveal the ratio of reactants necessary for a complete reaction.