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Question 6 (1 point) Caprylic acid has the formula CgH1602 and has a standard heat of...
Caprylic acid has the formula CgH1602 and has a standard heat of formation of -636 kJ/mol. If the standard heat of...
Caprylic acid has the formula CgH1602 and has a standard heat of formation of -636 kJ/mol. If the standard heat of formation for CO2(g) is -393.8 kJ/mol, and the standard heat of formation of H2O(l) is-289.8 kJ/mol, calculate the combustion enthalpy for caprylic acid, in kJ/mol. Your Answer: -441.4 kJ/mol
Question 2 (1 point) Saved The standard heat of combustion for naphthalene, C10Hg(s), is -5156.8 kJ...
Question 2 (1 point) Saved The standard heat of combustion for naphthalene, C10Hg(s), is -5156.8 kJ mol-1. Use this value and the given standard enthalpies of formation to calculate the standard enthalpy of formation of C1oHg(s) in kJ mol-1 H20() AHOf: H20() -285.9 kJ mol-1; -285.9 kJ mol-1. CO2(g) = -393.5 kJ mol-1 Hint: Hess' law; write the balanced chemical combustion equation and the chemical equation which defines the AHf of C10H8(s).
3. The standard enthalpy of formation of ethylbenzene (C3H10 (1)] is -12.5 kJ mol!. Calculate its...
3. The standard enthalpy of formation of ethylbenzene (C3H10 (1)] is -12.5 kJ mol!. Calculate its standard enthalpy of combustion. (AH®(CO2 (g)) = -393.51kJ mol', AH®, (H20 (1))= -285.83 kJ mol'). (Note: to solve this question you should write the balanced equation of ethylbenzene combustion reaction)
5. Heat of Reaction under standard conditions : Determine the amount of heat (in kJ) given...
5. Heat of Reaction under standard conditions : Determine the amount of heat (in kJ) given off, when 1.26 x 104 g of ammonia ( NH3 ) are produced according to the equation : N2 (g) + 3 H2 (g) → 2 NH3 (g) ....... AH ºrx = - 92.6 kJ Assume that the reaction occurs at Standard State conditions at 25 C. ANSWER : Total Heat Given Off: _ (units ?) 6. Standard Enthalpy of Formation and Reaction :...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...
ormation Reactions Review Constants Part B The standard heat of formation, AH is defined as the...
ormation Reactions Review Constants Part B The standard heat of formation, AH is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have AH O . Heat of formation values can be used to calculate the enthalpy change of any reaction. The combustion of propano, C, Hs. cocurs via the reaction CH, (B) +502 (6)+3CO2 (s) + 4H2O(g) with heat of formation...
6. Find the standard enthalpy of formation of ethylene, CH ) iven the following data: heat...
6. Find the standard enthalpy of formation of ethylene, CH ) iven the following data: heat of combustion of CH4(g) = -1411 kJ/mol: AH [CO2(g)] = -393.5 kd/mol; AHH.00) --285.8 kJ/mol. A) 52 kJ/mol D) 1.41 x 10 kJ/mol B) 87 kJ/mol E) 2.77 x 10 kJ/mol C) 731 kJ/mol PROBLEMS: Show all work for full credit. Point worth is in parentheses. A gas sample is held at constant pressure. The gas occupies 6,62 L of volume when the temperature...
It says the answer is supposed to be A) -126kJ/mol B) -2745.9kJ C)-440J/K 18.97 When 1.000...
It says the answer is supposed to be A) -126kJ/mol
B) -2745.9kJ
C)-440J/K
18.97 When 1.000 g of gaseous butane, C4H10, is burned at 25°C and 1.00 atm pressure, H2O(/) and CO2(g) are formed with the evolution of 49.50 kJ of heat. a Calculate the molar enthalpy of formation of butane. (Use enthalpy of formation data for H20 and CO2.) b AG of butane is -17.2 kJ/mol. What is AGo for the combustion of 1 mol butane? From a and...
The standard molar enthalpy of combustion, deltacHm, of C2H6 (g) is -1559.8 kJ/mol. 1. Use some...
The standard molar enthalpy of combustion, deltacHm, of C2H6 (g) is -1559.8 kJ/mol. 1. Use some of the following data to calculate the molar enthalpy of formation of C2H6(g) at 298.15 K 2. Calculate the molar enthalpy of combustion of ethane at 500K Table provided gives values of standard enthalpy of formation values at 298.15 K Substance deltafH (kJ*mol^-1) Cpm (J*K^-1*mol^-1) CO2 (aq) -413.8 N/A CO2 (g) -393.51 37.11 H2O (l) -285.83 75.291 H2O(g) -241.82 33.58 C2H6(g) to be determined...
Question 6 1 pts Which of the following reactions is a standard formation reaction (i.e. АHræn...
Question 6 1 pts Which of the following reactions is a standard formation reaction (i.e. АHræn = AH) at T = 298 K? O 2 Fe (s) + 1.5 O2() → Fe2O3(s) O N2(1) + 2 O2(1) ► N204(1) O CO(g) + 2H2(g) + CH3OH(1) O C(s, graphite) + H2(g) + O2(g) → C6H1206(s) O Cl2(g) + H2(g) →2 HCl(g) Question 4 1 pts A sample of 1.71 moles of a substance was burned in a constant pressure calorimeter. The...
Caprylic acid has the formula CgH1602 and has a standard heat of formation of -636 kJ/mol. If the standard heat of formation for CO2(g) is -393.8 kJ/mol, and the standard heat of formation of H2O(l) is-289.8 kJ/mol, calculate the combustion enthalpy for caprylic acid, in kJ/mol. Your Answer: -441.4 kJ/mol
Question 2 (1 point) Saved The standard heat of combustion for naphthalene, C10Hg(s), is -5156.8 kJ mol-1. Use this value and the given standard enthalpies of formation to calculate the standard enthalpy of formation of C1oHg(s) in kJ mol-1 H20() AHOf: H20() -285.9 kJ mol-1; -285.9 kJ mol-1. CO2(g) = -393.5 kJ mol-1 Hint: Hess' law; write the balanced chemical combustion equation and the chemical equation which defines the AHf of C10H8(s).
3. The standard enthalpy of formation of ethylbenzene (C3H10 (1)] is -12.5 kJ mol!. Calculate its standard enthalpy of combustion. (AH®(CO2 (g)) = -393.51kJ mol', AH®, (H20 (1))= -285.83 kJ mol'). (Note: to solve this question you should write the balanced equation of ethylbenzene combustion reaction)
5. Heat of Reaction under standard conditions : Determine the amount of heat (in kJ) given off, when 1.26 x 104 g of ammonia ( NH3 ) are produced according to the equation : N2 (g) + 3 H2 (g) → 2 NH3 (g) ....... AH ºrx = - 92.6 kJ Assume that the reaction occurs at Standard State conditions at 25 C. ANSWER : Total Heat Given Off: _ (units ?) 6. Standard Enthalpy of Formation and Reaction :...
ormation Reactions Review Constants Part B The standard heat of formation, AH is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have AH O . Heat of formation values can be used to calculate the enthalpy change of any reaction. The combustion of propano, C, Hs. cocurs via the reaction CH, (B) +502 (6)+3CO2 (s) + 4H2O(g) with heat of formation...
6. Find the standard enthalpy of formation of ethylene, CH ) iven the following data: heat of combustion of CH4(g) = -1411 kJ/mol: AH [CO2(g)] = -393.5 kd/mol; AHH.00) --285.8 kJ/mol. A) 52 kJ/mol D) 1.41 x 10 kJ/mol B) 87 kJ/mol E) 2.77 x 10 kJ/mol C) 731 kJ/mol PROBLEMS: Show all work for full credit. Point worth is in parentheses. A gas sample is held at constant pressure. The gas occupies 6,62 L of volume when the temperature...
It says the answer is supposed to be A) -126kJ/mol
B) -2745.9kJ
C)-440J/K
18.97 When 1.000 g of gaseous butane, C4H10, is burned at 25°C and 1.00 atm pressure, H2O(/) and CO2(g) are formed with the evolution of 49.50 kJ of heat. a Calculate the molar enthalpy of formation of butane. (Use enthalpy of formation data for H20 and CO2.) b AG of butane is -17.2 kJ/mol. What is AGo for the combustion of 1 mol butane? From a and...
Question 6 1 pts Which of the following reactions is a standard formation reaction (i.e. АHræn = AH) at T = 298 K? O 2 Fe (s) + 1.5 O2() → Fe2O3(s) O N2(1) + 2 O2(1) ► N204(1) O CO(g) + 2H2(g) + CH3OH(1) O C(s, graphite) + H2(g) + O2(g) → C6H1206(s) O Cl2(g) + H2(g) →2 HCl(g) Question 4 1 pts A sample of 1.71 moles of a substance was burned in a constant pressure calorimeter. The...
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