When i try to do this problem by simply using a mole ratio, wiley keeps saying it's wrong, what mistake am i making?
If 0.800 mol of liquid CS2 reacts stoichiometrically according to the balanced equation, how many moles of gaseous Cl2 are required?
CS2(l) + 3Cl2(g) → CCl4(l) + S2Cl2(l)
I just used a 1:3 mole ratio
0.800 mol CS2 requires 3 x 0.800 = 2.4 moles Cl2.
Based on the balanced equation, it is correct to use a mole ratio of 1:3 between CS2 and Cl2. However, to find the number of moles of Cl2 required, you need to multiply the given amount of CS2 (0.800 mol) by the appropriate mole ratio.
To do this, you can set up a proportion using the mole ratio:
(0.800 mol CS2) / (1 mol CS2) = (x mol Cl2) / (3 mol Cl2)
Cross-multiplying the proportion gives:
0.800 mol CS2 * 3 mol Cl2 = 1 mol CS2 * x mol Cl2
2.4 mol Cl2 = x mol Cl2
Therefore, to react stoichiometrically with 0.800 mol of CS2, you would need 2.4 moles of Cl2. This means that your calculation using the 1:3 mole ratio was correct, and the error might lie elsewhere.