The buildup of oxides of carbon in the atmosphere by the burning of fossil fuels is a driver for human's effect on the world's climate. A chemical solution to this buildup is the removal of these chemicals by reduction toreform small organic molecules like alkanes and alkenes.A chemist was investigating the removal of carbon dioxide by the following reaction:2 CO2(g) + 6 H2(g)C2H5OH(g) + 3 H2O(g)SpeciesAfH (kJ mol-1)S (J K*1mol-1)CO2(g)-393.5213.8H2(g)C2H5OH(g)H20(g)0.00131.1-277.4159.9-241.8188.8Using the data from the table above, calculate the enthalpy change, ArH, and entropy change, A,S, for this reaction. Show your working,

From the given data, □Hrxn= [total □Hf)products -[Total □Hf)reactant = (-277.4 -3×241.8)-(2× -393.5)…

Answered: SUK mol1) 213.8 131.1 159.9 188.8…

Science

Chemistry

SUK mol1) 213.8 131.1 159.9 188.8 calculate the enthalpy change, ArH, and entropy change, ArS, for this reaction.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 68E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...

See similar textbooks

Similar questions

In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
If nitric acid were sufficiently heated, it can be decomposed into dinitrogen pentoxide and water vapor: 2HNO3(l)N2O5(g)+H2O(g)Hrxn=+176kJ (a) Calculate the enthalpy change that accompanies the reaction of 1.00 kg HNO3 (). (b) Is heat absorbed or released during the course of the reaction?
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 3.06 g/L at 14 °C and 0.974 atm. Calculate the average molecular mass for this sample
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 1.43 g/L at 26 °C and 0.405 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of CH2F2 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111-trifluoroethane (C2H3F3) has a density of 2.39 g/L at 23 °C and 0.593 atm. 1. Calculate the average molecular mass for this sample. 2. Calculate the volume percentage of C2H3F3 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111- trifluoroethane ((C2H3F3) has a density of1.95 g/L at 23 °C and 0.432 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of C2H3F3 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 2.99 g/L at 22 °C and 0.810 atm. Calculate the average molecular mass for this sample.8.94×101 amu Calculate the volume percentage of CH2F2 in the sample.
Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 3.06 g/L at 14 °C and 0.974 atm. Calculate the volume percentage of CH2F2 in the sample.
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 63.5 mL water (where X is a hypothetical metal): X + 2 HCl → XCl2 + H2 In this process, the water temperature rose from 25.0 °C to 34.1 °C. If 0.00618 mol of "X" was consumed during the reaction, what is ΔrH of this reaction in kJ mol-1 with respect to "X"? The specific heat of water is 4.184 J g-1 °C-1 Express in 2 sig digs!
For hospital patients suffering from dehydration, it may be necessary to provide them with intravenous fluids. A common IV bag used for this purpose contains 4.00% (wv) glucose (MW = 180.16 g/mole) and 0.450% (w/v) of sodium chloride (MW = 58.44 g/mole). If you were attempting to prepare a standard 1.00 L bag of this solution starting from a stock solution containing 30.0% (w/v) glucose and 3.38% (w/v) sodium chloride, how many mL of the stock solution would you need? Hint: Only one calculation is needed.
An aqueous solution of cobalt(II) chloride, CoCl2, is made by dissolving 2.07 grams of cobalt(II) chloride in sufficient water in a 50.0 mL volumetric flask, and then adding enough water to fill the flask to the mark. What is the weight/volume percentage of cobalt(II) chloride in the solution? Weight/volume percentage = ______% How many grams of iron(III) fluoride, FeF3, are required to make a 6.28 %(w/v) aqueous solution in a 300. mL volumetric flask? ________g
The standard enthalpy change for the reaction of between sodium hydroxide and hydrochloric acid can be determined experimentally. What is the name given to the enthalpy change in this type of reaction? In one such experiment, 25cm3 each of solutions of sodium hydroxide and hydrochloric acid of concentration 1 mol/dm were mixed. The temperature rose from 270C to 340C. Calculate the standard enthalpy change for the reaction in KJ/mol. (Assume that the specific heat capacity of the solutions is 4.2KJkg-1K-1 and no heat is lost to the calorimeter)