Problem 8.45 reads: Carbon disulfide can be prepared from coke and elemental sulfur:
4C(s)+S8(s) --> 4CS2(l) deltaH=+358.8kJ
(a) 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 197g of carbon with an excess of sulfur.
(c) If the heat absorbed in the reaction was 415kJ, how much CS2 was produced?
Can someone walk me through the entire process of solving this, along with explanations? Thanks.
8.45 Preparation of Carbon Disulfide
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Re: 8.45 Preparation of Carbon Disulfide
a). You know from the balanced equation that +358.8kJ is absorbed for a reaction involving 1 mol of
. To find how much heat is absorbed for a reaction where 1.25 mol of
goes to completion, multiply 358.8kJ by 1.25.
b). To calculate the heat absorbed we need to know how many moles of C there are. Since the problem mentions there is an excess of sulfur, C is the limiting reagent. Divide 197g of C by the molar mass to obtain the moles of C. From the balanced equation you can see that for every 4 moles of C consumed in the reaction, 358.8kJ is absorbed. Multiply the moles of C by 358.8kJ/4mol to get the answer.
c). Calculate how many moles of
were produced by solving 415kJ/358.8kJ, then multiplying that quantity by 4 because remember 4 moles of
are produced in a reaction that absorbs 358.8kJ. Multiply the moles of
by the molar mass to get grams of
produced.
b). To calculate the heat absorbed we need to know how many moles of C there are. Since the problem mentions there is an excess of sulfur, C is the limiting reagent. Divide 197g of C by the molar mass to obtain the moles of C. From the balanced equation you can see that for every 4 moles of C consumed in the reaction, 358.8kJ is absorbed. Multiply the moles of C by 358.8kJ/4mol to get the answer.
c). Calculate how many moles of
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Re: 8.45 Preparation of Carbon Disulfide
a) (1.25mol S8) * (358.8 kJ/1mol S8) = 448.5 kJ
b) (197g C) * (1mol C/12.01g C) * (358kJ/4 mol C) = 1471.35 kJ
c) (415 kJ/358.8kJ) = (x mol CS2/4mol CS2); x = 4.63mol CS2
b) (197g C) * (1mol C/12.01g C) * (358kJ/4 mol C) = 1471.35 kJ
c) (415 kJ/358.8kJ) = (x mol CS2/4mol CS2); x = 4.63mol CS2
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Re: 8.45 Preparation of Carbon Disulfide
Leonardo Le Merle 1D wrote:a) (1.25mol S8) * (358.8 kJ/1mol S8) = 448.5 kJ
b) (197g C) * (1mol C/12.01g C) * (358kJ/4 mol C) = 1471.35 kJ
c) (415 kJ/358.8kJ) = (x mol CS2/4mol CS2); x = 4.63mol CS2
The question for the last partt asks for mass of CS2. So the answer needs to be in grams. Just multiply the moles by the grams of CS2 and get the answer in grams.
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