5C(s) + 2SO2(g) > CS2(l) + 4CO(g)

How many moles of carbon monoxide form at the same time that 0.246 mol CS2 forms?

0.984 mol CO

78

Well, aren't you asking some chemical recipe questions today? It seems like you're trying to balance a chemical equation. Let me put on my chemistry clown wig and help you out!

According to the balanced equation, for every 1 mole of CS2 that forms, 4 moles of CO are also produced. So, if you have 0.246 moles of CS2, you can expect to have (0.246 moles CS2) x (4 moles CO / 1 mole CS2) = 0.984 moles of CO.

So, approximately 0.984 moles of CO would form at the same time that 0.246 moles of CS2 forms. Keep those chemical reactions cooking!

To determine the number of moles of carbon monoxide (CO) formed when 0.246 moles of carbon disulfide (CS2) forms, we need to compare the stoichiometric coefficients of the balanced equation.

The balanced equation for the reaction is:

5C(s) + 2SO2(g) → CS2(l) + 4CO(g)

From the equation, we see that the stoichiometric coefficient of CS2 is 1, and the coefficient of CO is 4.

This means that for every 1 mole of CS2 formed, 4 moles of CO are also formed.

Therefore, if we have 0.246 moles of CS2, we can set up a proportion:

(0.246 mol CS2) / (1 mol CS2) = (x mol CO) / (4 mol CO)

To find the value of x (the number of moles of CO), we can cross-multiply and solve for x:

x = (0.246 mol CS2) * (4 mol CO) / (1 mol CS2)
x = 0.984 mol CO

So, 0.984 moles of carbon monoxide form at the same time that 0.246 moles of carbon disulfide forms.

1) Balance the equation.

It is balanced already.

2) From the balanced equation, determine the mole ratios for the compounds of interest.
1 mole CS2 = 4 moles CO

3) Determine how many moles you have of one of the two compounds of interest.
0.246 mol CS2

4) Multiple the moles of the one compound by the mole ration to find the equivalent (stoichiometrically) number of moles of the second.
0.246 mol CS2 (4 moles CO / 1 mole CS2) = ?