What is A, H° for the following chemical reaction?CO(g) + NH3 (9)→HCN(g)+ H2O(g)You can use the following table of standard heats of formation (Aş H°) to calculate the enthalpy of the given reaction.Standard Heat ofStandard Heat ofElement/ CompoundFormationElement/ CompoundFormation(kJ mol 1)(kJ mol-1)H(g)218N(g)473На (9)O2 (9)NH3 (9)-45.90O(g)249CO(g)-110.5H2O(g)-241.8C(g)71HCN(g)130.5C(s)HNO3 (ag)-206.6Express the standard enthalpy of reaction to three significant figures and include the appropriate units.

Heat of reaction is given by difference of energy of product 2 - energy of electron and heat of…

CO(g) + NH3(g)–→HCN(g)+H2O(g) can use the following table of standard heats of formation (A; H°) to calculate the enthalpy of the given reaction. Standard Heat of Standard Heat of Element/ Compound Formation (kJ mol 1) Element/ Compound Formation (kJ mol-1) H(g) 218 N(g) 473 На (9) O2 (9) NH3(9) -45.90 O(g) 249 CO(g) -110.5 H2O(g) -241.8 C(g) 71 HCN(g) 130.5 UNO (a) 206 6

CO(g) + NH3(g)–→HCN(g)+H2O(g) can use the following table of standard heats of formation (A; H°) to calculate the enthalpy of the given reaction. Standard Heat of Standard Heat of Element/ Compound Formation (kJ mol 1) Element/ Compound Formation (kJ mol-1) H(g) 218 N(g) 473 На (9) O2 (9) NH3(9) -45.90 O(g) 249 CO(g) -110.5 H2O(g) -241.8 C(g) 71 HCN(g) 130.5 UNO (a) 206 6

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.101PAE

See similar textbooks

Similar questions

Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(OH)2 Assuming that the temperature of both solutions was initially 25.0C and that the final mixture has a mass of 400.0 g and a specific heat capacity of 4.18 J/C g, calculate the final temperature of the mixture.
A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup calorimeter. As Ag2O(s) precipitates, the temperature of the solution increases from 23.78 C to 25.19 C. Assuming that the mixture has the same specific heat as water and a mass of 150 g, calculate the heat q. Is the precipitation reaction exothermic or endothermic?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
Nitric acid, HNO3, can be prepared by the following sequence of reactions: 4NH3(g)+5O2(g)4NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(l)+NO(g) How much heat is evolved when 1 mol of NH3(g) is converted to HNO3(l)? Assume standard states at 25 C.
Magnesium sulfate is often used in first-aid hot packs, giving off heat when dissolved in water. A coffee-cup calorimeter at 25C contains 15.0 mL of water at 25C. A 2.00-g sample of MgSO4 is dissolved in the water and 1.51 kJ of heat are evolved. (You can make the following assumptions about the solution: volume=15.0 mL, density=1.00 g/mL, specific heat=4.18J/gC.) (a) Write a balanced equation for the solution process. (b) Is the process exothermic? (c) What is qH2O? (d) What is the final temperature of the solution? (e) What are the initial and final temperatures in F?
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
A student performing a calorimetry experiment combined 100.0 ml. of 0.50 M HCI and 100.0 ml. of 0.50 M NaOH in a StyrofoamTM cup calorimeter. Both solutions were initially at 20.0 C, but when the two were mixed, the temperature rose to 23.2 C (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 ml of 0.50 M NaOH. WIII the AT observed be greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCI and 100.0 ml. of 1.00 M NaOH. Will the T observed be greater than, less than, or equal to that in the first experiment, and why?
The octane number of gasoline is based on a comparison of the gasolines behavior with that of 2,2,4-trimethylpentane, C8H18(), which is arbitrarily assigned an octane number of 100. The standard enthalpy of combustion of this compound is 5456.6 kJ/mol. (a) Write the thermochemical equation for the combustion of 2,2,4-trimethylpentane. (b) Use the standard enthalpies of formation in Appendix G to calculate the standard enthalpy of formation of 2,2,4-trimethylpentane.
A 250-g sample of water at 20.0C is placed in a freezer that is held at a constant temperature of 20.0C. Considering the water as the system, answer the following questions: a What is the sign of qsys for the water after it is placed in the freezer? b After a few hours, what will be the state of the water? c How will the initial enthalpy for the water compare with the final enthalpy of the water after it has spent several hours in the freezer? d What will the temperature of the water be after several hours in the freezer?