How many moles of carbon monoxide gas are produced from the reaction of 5.00 moles of SnO2(s) with 9.00 moles of carbon according to the equation below?



SnO2(s) + 2C(s) → Sn(s) + 2CO(g)

Question 28 options:

4.50 mol


9.00 mol


18.0 mol


5.00 mol


7.50 mol

Well, it looks like we have to balance the equation first. So let's see...

SnO2(s) + 2C(s) -> Sn(s) + 2CO(g)

Alright, now we can compare the coefficients to determine the ratio of moles produced. From the balanced equation, we can see that 2 moles of CO are produced for every 1 mole of SnO2 that reacts.

So if we start with 5.00 moles of SnO2, we can expect to produce 2 times that amount of CO, which is 10.00 moles. But wait, we also have 9.00 moles of carbon, and we know that for every mole of carbon, we produce 2 moles of CO. So that means we can produce an additional 2 times 9.00 moles of CO, which is 18.00 moles.

Adding these two amounts together, we get a total of 10.00 moles + 18.00 moles, which is 28.00 moles of CO.

Oh wait, I made a mistake. I was so busy calculating, I forgot to bring in the humor! Well, let's just say the answer is "CO-lossal" at 28.00 moles! Eh? Eh?

So the correct answer is 28.00 moles of CO.

To determine the number of moles of carbon monoxide gas produced, you need to use the stoichiometry of the balanced chemical equation. According to the equation:

SnO2(s) + 2C(s) → Sn(s) + 2CO(g)

The ratio between SnO2 and CO is 1:2. This means that for every 1 mole of SnO2 reacted, 2 moles of CO are produced.

Given that you have 5.00 moles of SnO2, you can determine the amount of CO produced by multiplying the mole ratio by the number of moles of SnO2:

5.00 mol SnO2 x (2 mol CO/1 mol SnO2) = 10.0 mol CO

Therefore, the number of moles of carbon monoxide gas produced is 10.0 mol.

To find the number of moles of carbon monoxide gas produced, we need to use the stoichiometric coefficients from the balanced chemical equation.

According to the balanced equation:
1 mole of SnO2 reacts with 2 moles of carbon to produce 2 moles of CO gas.

We are given:
5.00 moles of SnO2
9.00 moles of carbon

From the given information, we can determine the limiting reactant by comparing the number of moles of each reactant to their corresponding stoichiometric coefficients. The reactant that produces the fewer moles of product will be the limiting reactant.

Using the stoichiometry:
5.00 moles SnO2 x (2 moles CO / 1 mole SnO2) = 10.00 moles CO
9.00 moles C x (2 moles CO / 1 mole C) = 18.00 moles CO

Since the theoretical yield of carbon monoxide gas is determined by the limiting reactant, which is carbon in this case, the maximum number of moles of CO that can be produced is 18.00 mol.

Therefore, the correct answer is option "18.0 mol".

5 mols SnO2 reqires 10 mols C

but we only have 9
9 mols C require 4.5 mols SnO2
and yield 9 mols CO with half a mol SnO2 left over
The 10 mols CO will kill you.