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Adam Perez
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Postby Adam Perez » Thu Jan 19, 2017 10:41 pm

8.45 Carbon disulfi de can be prepared from coke (an impure form of carbon) and elemental sulfur: 4 C1s2  S81s2¡4 CS21l2 ¢H°  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.

I am so confused as to how to do the first part of this problem. I saw the solution but it doesnt make sense as to how they got the equation to solve part a.

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Re: 8.45

Postby Jeffrey_Huang_2K » Thu Jan 19, 2017 10:53 pm

The reaction enthalpy of deltaH = +358.8 kJ specifically describes the situation where one mol of S8 reacts. When 1.25 mol is reacted, then the reaction enthalpy (notice it is positive so heat is absorbed) is also multiplied by this new amount of reactant.

(358.8 kJ)(1.5 mol S8) = 448.5 kJ

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Re: 8.45

Postby GabrielaGutierrez2A » Sat Jan 28, 2017 4:30 pm

Does anyone know how to do part b?

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Re: 8.45

Postby stephanieyang_3F » Sat Jan 28, 2017 5:37 pm

Part B is basically asking how much heat is absorbed when that much amount of carbon reacts with S8. Since sulfur is in excess, the amount of carbon in the reaction goes to completion, which means it will determine the reaction's yield of heat. Since the original reaction said 358 kJ is associated with 4 moles of C reacting with 1 mole of S8, (also means 358 kJ is absorbed by that many moles of reactants reacting together), you'd find the amount of heat absorbed when you input 197 g of C by multiplying the moles of C (197g C to moles) by the reaction's (358kJ/4moles of C). The 358kJ is the amount of heat absorbed when there's 4 moles of C and you wanna find out the amount of heat absorbed when there's 197 g of C.

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