4. Electrolysis dissociates liquid water molecules into hydrogen and oxygen gases with the use of electricity. Which thermochemical equation represents the reaction? H(g) + 0,g) a. H,O() AH=-285.8 kJ/mol b. 2H,) + 0,(g) AH=571.6 kJ/mol AH= 285.8 kJ/mol AH=571.6 kJ/mol 5. Nitrogen dioxide (NO,) is cooled to produce dinitrogen tetroxide (N,O,). Which thermo- - 2H,O() H,O(g) H(g) + 0,(g) C. d. 2H,O() 2H,(g) + 0,(g) chemical equation represents the reverse reaction? AH? of NO,=33.9 kJ/mol AH?of N,O,=9.2 kJ/mol N,O.() + 2NO,(g) AH=24.7 kJ/mol a. b. NO(g) → 2NO,(g) AH=58,6 kJ/mol 2NO,() N,0(g) d. 2NO,g) How much heat does a 15-gram piece of aluminum metal release as it cools from 260°C to AH=-24.7 kJ/mol с. → N,O.() AH=-58,6 kJ/mol 35°C? 4.18 J b. 3027 J a. 3375 J С. d. 6054 J

4. Electrolysis dissociates liquid water molecules into hydrogen and oxygen gases with the use of electricity. Which thermochemical equation represents the reaction? H(g) + 0,g) a. H,O() AH=-285.8 kJ/mol b. 2H,) + 0,(g) AH=571.6 kJ/mol AH= 285.8 kJ/mol AH=571.6 kJ/mol 5. Nitrogen dioxide (NO,) is cooled to produce dinitrogen tetroxide (N,O,). Which thermo- - 2H,O() H,O(g) H(g) + 0,(g) C. d. 2H,O() 2H,(g) + 0,(g) chemical equation represents the reverse reaction? AH? of NO,=33.9 kJ/mol AH?of N,O,=9.2 kJ/mol N,O.() + 2NO,(g) AH=24.7 kJ/mol a. b. NO(g) → 2NO,(g) AH=58,6 kJ/mol 2NO,() N,0(g) d. 2NO,g) How much heat does a 15-gram piece of aluminum metal release as it cools from 260°C to AH=-24.7 kJ/mol с. → N,O.() AH=-58,6 kJ/mol 35°C? 4.18 J b. 3027 J a. 3375 J С. d. 6054 J

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU5: Fire: Energy , Thermodynamics, And Oxidation-reduction

Section: Chapter Questions

Problem 4STP

See similar textbooks

Similar questions

A calorimeter contains 72.0g of water at 19.2C. A 141-g piece of tin is heated to 89.0C and dropped into the water. The entire system eventually reaches 25.5C. Assuming all of the energy gained by the water comes from the cooling of the tin-no energy loss to the calorimeter or the surroundings-calculate the specific heat of the tin.
sUse information from Figure 15.24 to calculate howmuch heat is required to vaporize 4.33 mol of waterat 100°C.
ou place hot metal into a beaker of cold water. ol type='a'> Eventually what is true about the temperature of the metal compared to that of the water? Explain why this is true. i>Label this process as endothermic or exothermic if we consider the system to be the metal. Explain. the water. Explain.
Are changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?
If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?
A 0.500-g sample of KCl is added to 50.0 g of water in a calorimeter (Figure 5.12). If the temperature decreases by 1.05 °C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the specific heat of the resulting solution is 4.18 J/g °C? Is the reaction exothermic or endothermic?
The enthalpy of vaporization of water is larger than its enthalpy of fusion. Explain why.
If the 3.21 g of NH4NO3 in Example 5.6 were dissolved in 100.0 g of water under the same conditions, how much would the temperature change? Explain your answer.
Describe, on both a microscopic and a macroscopic basis, what happens to a sample of water as it is cooled from room temperture to 50Cbelow its normal freezing point.
Consider the following reaction for the combustion of octane, C8H18: msp;2C8H18(l)+25O2(g)16CO2(g)+18H2O(l) at volume of oxygen gas at STP would be needed for the complete combustion of 10.0gof octane?
What is the energy change when the temperature of 10.1g of solid silver is decreased from 38.1C to 23.6C?
Find the quantity of energy released in joules as 467g of zinc cools from 68C to 31C.