Can you please provide detailed answers to the below question
![Question B1 (a) Which enthalpies of formation must be known to find the enthalpy of reaction (ArH) for the reaction given below? CO2(g)+ H2(g) CO(g) + H20(g) Explain your answer in terms of Hesss law. 2 marks] (b) Enthalpy is a state function. Please explain what is meant by a state function. [1 mark] (c) Name two other thermodynamic functions that are state functions. [1 mark] (d) Which thermodynamic function can be used to calculate the equilibrium constant? [1 mark]](http://img.homeworklib.com/questions/349ff300-1318-11ec-a6be-476d268b109d.png?x-oss-process=image/resize,w_560)
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Question B1 (a) Which enthalpies of...
Given the enthalpies of combustion of propane (C3Hg), carbon and hydrogen, C3H3(g) + 5 O2(g) +...
Given the enthalpies of combustion of propane (C3Hg), carbon and hydrogen, C3H3(g) + 5 O2(g) + 3 CO2(g) + 4 H20(1) AH° = -2219.9 kJ C(s) + O2(g) + CO2(8) AH° = -393.5 kJ 2 H2(g) + O2 + 2 H2O(1) AH° = -571.6 kJ Calculate the enthalpy of formation of propane. The reaction is shown below. 3 C(s) + 4H2(g) → C3H3(g)
need help with 2. Use the following enthalpies of formation to calculate an approximate enthalpy of...
need help with
2. Use the following enthalpies of formation to calculate an approximate enthalpy of reaction, AHrxn for: (5 pts) C3H8 (g) + 502 (g) → 3CO2 (g) + 4 H20 (1) C(s) + O2 (g) - CO2 (g); AH = - 393.5 kJ/mol H2(g) + 42 02 (g) - H20 (1); AH = - 285.5 kJ/mol 3 C(s) + 4 H2(g) → C3H8 (g); AH r = - 103.8 kJ/mol
which of the following statements is/are true concerning a state function Using the standard enthalpies of...
which of the following statements is/are true concerning a
state function
Using the standard enthalpies of formation listed below, determine the standard enthalpy change for the following reaction: Fe2O3(s) + 3CO(g) ---> 2Fe(s) + 3C02() AH°-m AH" for Fe2O3(s) --824.2 kJ/mol AH® for CO(g) = -110.5 kJ/mol AH", for CO2(g) - -393.5 kJ/mol
1. The enthalpies of the following reactions can be measured. CH, (g) + 20, (g) CO2(g)...
1. The enthalpies of the following reactions can be measured. CH, (g) + 20, (g) CO2(g) + 2H,0 (g) AH = -802.4 kJ CH,OH (g) +/, 0, (g) CO2(g) + 2H,0 (g) AH = -676 kJ Use these values and Hess's law to determine the enthalpy change for the reaction CH, (g) +'/20 (8) CH,OH(g)
2. The enthalpies of the following reactions can be measured. CH, (g) + 302 (8) 200,...
2. The enthalpies of the following reactions can be measured. CH, (g) + 302 (8) 200, (g) + 2H,0 (1) AH = -1411.1 kJ CH,OH (1) + 302 (9) 2002 (9) + 3H20 (1) AH° = -1367.5 kJ Use these values and Hess's law to determine the enthalpy change for the reaction CH, (g) + H20 (1) - CHOH (1)
Using Hess's Law to Calculate a Standard Enthalpy of Formation On the Solution Calorimetry Lab Report...
Using Hess's Law to Calculate a Standard Enthalpy of Formation On the Solution Calorimetry Lab Report Form, vou will be asked to calculate a standard enthalpy of formation for magnesium oxide based on your experimental results. Below is an example of how to do this type of calculation. Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using the following thermochemical equations: 4 B(s) + 3 O2(g)-> 2 B2O3(s) 2 H2(g) + O2(g) > 2 H20(0) B2H6(8) +3 O2(g)...
Consider the reaction: 2 BsHs (I)12 02 (g) (a) Use the standard enthalpies of formation found...
Consider the reaction: 2 BsHs (I)12 02 (g) (a) Use the standard enthalpies of formation found in Appendix B of the textbook to calculate the enthalpy change of the reaction. The standard enthalpy of formation of BsH, (I) is 73.2 kl/mol. 5 B2Os (s) +9 H2O (I) (b) Predict the sign of the entropy change and provide the two reasons likely to have made the biggest impact on the entropy change (and upon which you based your prediction). (c) Based...
Question 9 (1 point) Using enthalpies of formation on our data table, which is closest to...
Question 9 (1 point) Using enthalpies of formation on our data table, which is closest to the enthalpy change for the reaction below? 2 NO2 (g)N204 (g) 42.48 kJ 24.01 kJ 57.93 kJ 24.01 kJ 57.93 kJ
Calculate [delta H0 f] in kJ for the equation below using the standard enthalpies of formation...
Calculate [delta H0 f] in kJ for the equation below using the
standard enthalpies of formation seen in the image:
Testbank, Question 6.123 Using the standard enthalpies of formation, AH : CO(g) = -110.5 kJ mol-1 CO2(g) = -393.5 kJ molt SO2(g) = -296.9 kJ molt SO3(g) = -395.2 k) mol-1 calculate AH reaction for CO2(g) + SO2(g) — 503(9) + CO(g)
| 10. + -1 points ChangWA12 6.СМ.011. My Notes Ask Your Teacher The combustion reaction of...
| 10. + -1 points ChangWA12 6.СМ.011. My Notes Ask Your Teacher The combustion reaction of butane is as follows. C4H10(9)13/2 02(9)-4 CO2(g) 5 H20(0) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g)-. CO2(g) reaction (2): 21/2 02(9) H20UAH--285.8 kJ/mo reaction (3): 4 C(s) + 5 H2(g)- + C4H10(g) H-_1257 krmol H--393.5 kJ/mol kJ/mol Supporting Materials Periodic Table Constants and Factors Supplemental Data
Given the enthalpies of combustion of propane (C3Hg), carbon and hydrogen, C3H3(g) + 5 O2(g) + 3 CO2(g) + 4 H20(1) AH° = -2219.9 kJ C(s) + O2(g) + CO2(8) AH° = -393.5 kJ 2 H2(g) + O2 + 2 H2O(1) AH° = -571.6 kJ Calculate the enthalpy of formation of propane. The reaction is shown below. 3 C(s) + 4H2(g) → C3H3(g)
need help with
2. Use the following enthalpies of formation to calculate an approximate enthalpy of reaction, AHrxn for: (5 pts) C3H8 (g) + 502 (g) → 3CO2 (g) + 4 H20 (1) C(s) + O2 (g) - CO2 (g); AH = - 393.5 kJ/mol H2(g) + 42 02 (g) - H20 (1); AH = - 285.5 kJ/mol 3 C(s) + 4 H2(g) → C3H8 (g); AH r = - 103.8 kJ/mol
which of the following statements is/are true concerning a
state function
Using the standard enthalpies of formation listed below, determine the standard enthalpy change for the following reaction: Fe2O3(s) + 3CO(g) ---> 2Fe(s) + 3C02() AH°-m AH" for Fe2O3(s) --824.2 kJ/mol AH® for CO(g) = -110.5 kJ/mol AH", for CO2(g) - -393.5 kJ/mol
1. The enthalpies of the following reactions can be measured. CH, (g) + 20, (g) CO2(g) + 2H,0 (g) AH = -802.4 kJ CH,OH (g) +/, 0, (g) CO2(g) + 2H,0 (g) AH = -676 kJ Use these values and Hess's law to determine the enthalpy change for the reaction CH, (g) +'/20 (8) CH,OH(g)
2. The enthalpies of the following reactions can be measured. CH, (g) + 302 (8) 200, (g) + 2H,0 (1) AH = -1411.1 kJ CH,OH (1) + 302 (9) 2002 (9) + 3H20 (1) AH° = -1367.5 kJ Use these values and Hess's law to determine the enthalpy change for the reaction CH, (g) + H20 (1) - CHOH (1)
Using Hess's Law to Calculate a Standard Enthalpy of Formation On the Solution Calorimetry Lab Report Form, vou will be asked to calculate a standard enthalpy of formation for magnesium oxide based on your experimental results. Below is an example of how to do this type of calculation. Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using the following thermochemical equations: 4 B(s) + 3 O2(g)-> 2 B2O3(s) 2 H2(g) + O2(g) > 2 H20(0) B2H6(8) +3 O2(g)...
Consider the reaction: 2 BsHs (I)12 02 (g) (a) Use the standard enthalpies of formation found in Appendix B of the textbook to calculate the enthalpy change of the reaction. The standard enthalpy of formation of BsH, (I) is 73.2 kl/mol. 5 B2Os (s) +9 H2O (I) (b) Predict the sign of the entropy change and provide the two reasons likely to have made the biggest impact on the entropy change (and upon which you based your prediction). (c) Based...
Question 9 (1 point) Using enthalpies of formation on our data table, which is closest to the enthalpy change for the reaction below? 2 NO2 (g)N204 (g) 42.48 kJ 24.01 kJ 57.93 kJ 24.01 kJ 57.93 kJ
Calculate [delta H0 f] in kJ for the equation below using the
standard enthalpies of formation seen in the image:
Testbank, Question 6.123 Using the standard enthalpies of formation, AH : CO(g) = -110.5 kJ mol-1 CO2(g) = -393.5 kJ molt SO2(g) = -296.9 kJ molt SO3(g) = -395.2 k) mol-1 calculate AH reaction for CO2(g) + SO2(g) — 503(9) + CO(g)
| 10. + -1 points ChangWA12 6.СМ.011. My Notes Ask Your Teacher The combustion reaction of butane is as follows. C4H10(9)13/2 02(9)-4 CO2(g) 5 H20(0) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g)-. CO2(g) reaction (2): 21/2 02(9) H20UAH--285.8 kJ/mo reaction (3): 4 C(s) + 5 H2(g)- + C4H10(g) H-_1257 krmol H--393.5 kJ/mol kJ/mol Supporting Materials Periodic Table Constants and Factors Supplemental Data
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