textbook 4.d 1

[Jenna 1G]

4D.1 Carbon disulfide can be prepared from coke (an impure form of carbon) and elemental sulfur:4C(s)+S8(s)→4 CS2(l)ΔH°=+358.8 kJ How much heat is absorbed in the reaction of 1.25 mol S8 at constant pressure? (b) Calculate the heat absorbed in the reaction of 197 g of carbon with an excess of sulfur. (c) If the heat absorbed in the reaction was 415 kJ, how much CS2 was produced?

I was wondering what equations I needed to know to solve this problem.

[Arjun_Anumula_3E]

All you need is an understanding of stoichiometry here. So they tell us that 358.8 kJ of Energy is absorbed/required per mole of this reaction. So for the first part, since there is 1 mol of s8/mol of rxn, we can just multiply the 358.8 kJ /mol rxn * 1.25 mol rxn to get 448.5 kJ. Do the same stoichiometry type calculations for part b and c.