At 25 °C, the following reaction is CH4(9) + 2O2(g) + CO2(g) + 2 H2O(1) Nonspontaneous...
Consider following chemical reactions: 1) CH2(g) + 2O2(g) → CO2(g) + 2H20(1) 2) C(s) + O2(g) → CO2(g) 3) 2C(s) + O2(g) 200(g) 4) 3C(s) + 2H2O(l) → CH4(9) + CO2(g) H2O(l) indicates that H2O 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.
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
Use Hess's law and the following data CH4(g) + 2O2(g) → CO2(g) + 2 H2O(g) AH° = -802 kJ mol-1 CH4(8) + CO2(g) —> 2CO(g) + 2 H2(g) AFH° = +247 kJ mol-1 CH4(g) + H2O(g) –> CO(g) + 3H2(g) AFH° = +206 kJ mol-1 to determine A.Hº for the following reaction, an important source of hydrogen gas CH4(8) + +02(8) — CO(g) + 2 H2(8)
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...
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
Calculate the enthalpy of the following reaction: C (s) + 2 H2 (g) --> CH4 (g) Given: C (s) + O2 (g) --> CO2 ΔH = -393 kJ H2 + 1⁄2O2 --> H2O. ΔH = -286 kJ CH4 + 2O2 --> CO2 + 2H2O ΔH = -892 kJ
The thermochemical equation of combustion of methane is: CH4(g) + 2O2(g) → CO2(g) + 2 H2O(l) ΔΗ =-890.3 kJ 1. Calculate the AH when 5.00 g CH4 react with excess of oxygen. 2. Calculate AH when 2L CH4 at 49 °C and 782 mmHg react with an excess of oxygen 3. Calculate AH when 2L CH4 react with L O2 in a reaction vessel kept at 49 °C and 782 mmHg.
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 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.
Calculate the standard-state entropy for the following reaction: 1 CH4(g) + 2 O2(g) ⟶ 1 CO2(g) + 2 H2O(l) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. Formula S∘ J/(K⋅mol) CO2(g) 214 H2O(l) 189 CH4(g) 186 O2(g) 205