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
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.
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
AU for the reaction CH4 (8) + 2O2(g) - CO2(8) + 2H2O(l) in kJ at 298 K is AH(CH,) =-74.6kJ / mol AH (0) = -393.5kJ / mol AH,(4,0) =-285.8kJ / mol 1 A. -885.5 kJ B.668 kJ C. 885.5 kJ D.-668 kJ
CO2(g) H2O(g) CH4(g) +17 AHp/kJ mol -394 -242 These data can be used to calculate the enthalpy change for the reaction in part (b). (ii) Use the data from the formation table above to calculate the standard enthalpy of combustion of methane. 13 marke
Calculate ΔrH for the following reaction: CH4(g)+2O2(g)→CO2(g)+2H2O(l) Use the following reactions and given ΔrH's. CH4(g)+O2(g)→CH2O(g)+H2O(g), ΔrH = -284 kJmol−1 CH2O(g)+O2(g)→CO2(g)+H2O(g), ΔrH = -527 kJmol−1 H2O(l)→H2O(g), ΔrH = 44.0 kJmol−1
2. Given the following reaction: 2CH2OH(g) + 302(g) → 2CO2(g) + 4H2O(g) Delta Gº Kj/mol -163 CH2OH O, CO2 H20 -394 -229 What is Delta G for the reaction
In the reaction CO2(g) + 2H2O(g) ? CH4(g) + 2O2(g) the initial rate of change in the concentration of CO2 is ?3.2 × 10?5 M s?1. What are the initial rates of change in the concentration of the other three substances in the reaction mixture?
Given the following equilibrium equations and their corresponding equilibrium constants: 2CO2 (g)+H2O(g)⇌2O2 (g)+CH2CO(g) Kc=6.1x108 CH4(g)+2O2(g)⇌CO2 (g)+2H2O(g) Kc=1.2x1014 Find Kc for the reaction: CH4(g) + CO2(g) ⇌ CH2CO (g) + H2O (g) 2 of 5 .. .........e following equilibrium equations and their corresponding equilibrium constants: 2 CO2 (g) + H20 (g) – 202 (g) + CH2CO (g) Kc = 6.1 x 108 CH2(g) + 2 O2(g) - CO2 (g) + 2 H2O(g) Kc = 1.2 x 1014 Find Kc for the...
What mass of natural gas (CH4) must you burn to emit 258 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ