Homework Answers
Answer : a) -885.5 KJ/mol
Formula used :
∆H°f (rxn) = ∆H°f(products) - ∆H°f (reactants)
∆U = ∆H - ∆ng RT ,
where ∆ng = moles of gaseous product - moles of gaseous reactant
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AU for the reaction CH4 (8) + 2O2(g) - CO2(8) + 2H2O(l) in kJ at 298...
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and...
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g).
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and...
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g): 572 kJ -801 kJ -572 kJ 801 kJ
CH4(g) + 2O2(g) CO2(g) + 2H2O(l) ΔHo = -890.5 kJ. What would be the ΔHo...
CH4(g) + 2O2(g) CO2(g) + 2H2O(l) ΔHo = -890.5 kJ. What would be the ΔHo for the reaction ½ CH4(g) + O2(g) ½ CO2(g) + H2O(l) What would be the ΔHo for the reaction ½ CH4(g) + O2(g) ½ CO2(g) + H2O(l) What would be the ΔHo for ½ CO2(g) + H2O(l) ½ CH4(g) + O2(g)
CH4(g) + 2O2(g), AH° = 803 kJ which of the following For the following reaction, CO2(g)...
CH4(g) + 2O2(g), AH° = 803 kJ which of the following For the following reaction, CO2(g) + 2H2O(g) = will increase K? Select one: O a. increase the temperature of system O b. none of the above O c. decrease number of moles of methane O d. all of the above O e increase volume of system
Use the example shown to calculate the reaction enthalpy, delta H, for the following reaction: CH4(g)+2O2(g)->CO2(g)2H2O(l)....
Use the example shown to calculate the reaction enthalpy, delta H, for the following reaction: CH4(g)+2O2(g)->CO2(g)2H2O(l). Use the series of reaction that follows: 1. C(s)+2H2(g)-> CH4(g), delta H= -74.8 kJ 2. C(s)+O2(g)->CO2(g), delta H= -393.5 kJ 3. 2H2(g)+O2(g)-> 2H2O(g), delta H= -484.0 kJ 4. H2O(l)->H2O(g), delta H= 44.0 kJ
CH_(g) + 2O2(g) → CO2(g)+ 2H2O(1) AH = -890.4 kJ When 1 mole of CO2(g) is produced, what is the enthalpy change? Wh...
CH_(g) + 2O2(g) → CO2(g)+ 2H2O(1) AH = -890.4 kJ When 1 mole of CO2(g) is produced, what is the enthalpy change? When 3 mol of O, is reacted with an excess of CH4, what is the enthalpy change? When 1 mole of H,O(l) is produced, what is the enthalpy change?
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The...
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
please help Consider following chemical reactions: 1) CH.(g) + 2O2(g) → CO2(g) + 2H2O(1) 2) C(s) + O2(g) → CO2(g) 3)...
please help
Consider following chemical reactions: 1) CH.(g) + 2O2(g) → CO2(g) + 2H2O(1) 2) C(s) + O2(g) → CO2(g) 3) 2C(s) + O2(g) - 200(g) 4) 3C(s) + 2H2O) CH4(g) + 2COg) H2O(l) indicates that H20 is in liquid state. If the Enthalpy of reaction for reaction 1, 2, and 3 are -890.4kj, -393.5kj and - 221.Okj respectively; try to figure out the Enthalpy of reaction for reaction 4. Please show your work.
Consider the exothermic reaction CH4(g)+2O2(g)→CO2(g)+2H2O(g) Calculate the standard heat of reaction, or ΔH∘rxn, for this reaction...
Consider the exothermic reaction CH4(g)+2O2(g)→CO2(g)+2H2O(g) Calculate the standard heat of reaction, or ΔH∘rxn, for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure form is considered to be zero. Reactant or product ΔH∘f (kJ/mol) CH4(g) -201 CO2(g) -393.5 H2O(g) -241.8 Express your answer to four significant figures and include the appropriate units.
The equilibrium constant expression K c for the reaction CH4 (g) + 2O2 (g) <--> CO2...
The equilibrium constant expression K c for the reaction CH4 (g) + 2O2 (g) <--> CO2 (g) + 2H2O (g) is __________. A. Kc = [CO2][H2O]/[CH4][O2] B. Kc = [CO2][H2O]2/[CH4][O2]2 C. Kc = [CH4][O2]/[CO2][H2O] D. Kc = [CH4][O2]2/[CO2][H2O]2
CH4(g) + 2O2(g), AH° = 803 kJ which of the following For the following reaction, CO2(g) + 2H2O(g) = will increase K? Select one: O a. increase the temperature of system O b. none of the above O c. decrease number of moles of methane O d. all of the above O e increase volume of system
CH_(g) + 2O2(g) → CO2(g)+ 2H2O(1) AH = -890.4 kJ When 1 mole of CO2(g) is produced, what is the enthalpy change? When 3 mol of O, is reacted with an excess of CH4, what is the enthalpy change? When 1 mole of H,O(l) is produced, what is the enthalpy change?
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
please help
Consider following chemical reactions: 1) CH.(g) + 2O2(g) → CO2(g) + 2H2O(1) 2) C(s) + O2(g) → CO2(g) 3) 2C(s) + O2(g) - 200(g) 4) 3C(s) + 2H2O) CH4(g) + 2COg) H2O(l) indicates that H20 is in liquid state. If the Enthalpy of reaction for reaction 1, 2, and 3 are -890.4kj, -393.5kj and - 221.Okj respectively; try to figure out the Enthalpy of reaction for reaction 4. Please show your work.
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