Using the data provided and assuming complete combustion, estimate the mass of CO2 and SO2 produced per day by a 1000MW electrical power plant burning bituminous coal from West Virginia. Mass composition of coal: 78.0% C, 6.0% H, 7.0% O, 1.0% N, 5.0% S and 3.0% inorganics. Heating value of coal = 29.O MJ kg-1. Overall efficiency of plant = 35%. Report final answer in units of tonne/day. Answer: CO2 = 24 300 t/day, SO2 = 850 t/day ***

Using the data provided and assuming complete combustion, estimate the mass of CO2 and SO2 produced per day by a 1000MW electrical power plant burning bituminous coal from West Virginia. Mass composition of coal: 78.0% C, 6.0% H, 7.0% O, 1.0% N, 5.0% S and 3.0% inorganics. Heating value of coal = 29.O MJ kg-1. Overall efficiency of plant = 35%. Report final answer in units of tonne/day. Answer: CO2 = 24 300 t/day, SO2 = 850 t/day ***

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 52E: Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00...

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Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00 kcal/mol) was used in household refrigerators. What mass of SO2 must be evaporated to remove as much heat as evaporation of 1.00 kg of CC12F2 (enthalpy of vaporization is 17.4 kJ/mol)? The vaporization reactions for SO2 and are SO2(l)SO2(g) and CCl2F(l)CCl2F2(g), respectively.
When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
Methanol is known to be the simplest alcohol, and is used as an antifreeze agent, a solvent, a fuel anda denaturant for ethyl alcohol. It is also known as “wood spirit”, as it is obtained from the pyrolysis ofwood. Methanol burns in air to produce CO2(g) and H2O(l). The chemical reaction is: 2CH3OH (ℓ)+ 3O2 (g) à 2CO2 (g) + 4H2O (ℓ)Calculate the enthalpy change for the reaction using the standard enthalpies of formation are found onthe chart provided.
3. (a) jf 10.0 mjL of H2jSO4 (sp. jr. 1.50, containing 48.7% of combined SO3 by weight) is diluted to 400 mL, what is the normality of the solution as an acid? (b) What volume of 6.00 M H2SO4 should be added to this in order to make the resulting mixture 1.00N as an acid? FW's : H2SO4 = 98; SO3 = 80 %3D
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