Assuming Kc3 to be equilibrium constant.
Kc for required equation = 1.21 x 1029
7. Given the equilibrium constants for the following reactions, 2 CH4 (g) = C2H6 (g) +...
Given the following information: 2CH4(9) C2H6(g) + H2(g) K1 = 9.5 x 10-13 CH4(9) + H2O(g) - CH3OH(g) + H2(g) K2 = 2.8 * 10-21 Calculate the the value of K for the reaction: C2H6(g) + 2H2O(g) = 2CH3OH(g) + H2(g) K3 = ?
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...
Given the equilibrium constants for the following reactions: 2H2(g) + O2(g) → 2H2O(g) K1 = 3.74 x 1026 H2(g) + Cl2(g) → 2HCl(g) K2 = 9.73 x 1012 calculate the equilibrium constant for the reaction below. 4HCl(g) + O2(g) → 2Cl2(g) + 2H2O(g)
Given that K1 and K2 are the respective equilibrium constants for the two reactions CO2(g) + H2(g) = CO(g) + H2O(l) K1 = 3.08×10-4 CdO(s) + H2(g) = Cd(s) + H2O(l) K2 = 40.7 Determine the equilibrium constant for the reaction CO(g) + CdO(s) = CO2(g) + Cd(s) K =
Calculate the equilibrium for the reaction given the system CH4 + 2 H2O -----------> CO2 + 4H2 at equilibrium, we find that 96.8 g of co2 along with 8.0 H2 and 99.2 of CH4 and 54 g of H20 were present in a 15.0 L container Calculate the equilibrium for the reaction [hint: convert the given values to molarity first]
02 INTRO UNIV CHEM Il (LEC D1 Wi18) Te left Use the following equilibrium constants co2(g) + H2(g) <→ CO(g) + H2O(g) K,(400 K) 6.5 x 10 E(s) + 1 /202(g) <==> CO(g) K,(400 K) 1.3 x 1019 CO(g)+ 1/2 O2(g)CO2(g) K,(400 K) 2.8 x 102 CO(g) + 2 H2(g)CH3OH(g) K,(400 k) -2.3 H2(g) + 1 /202(g)-> H2O(g) (400 K)-1.8 x 1029 to determine the equilibrium constant for the following reaction. (You will not need to use all of the...
Here are four different comments: (1) C (s) + H2 (g) => CH4 (g) (2) C2H6 (g) + O2 (g) => CO2 (g) + H2O (l) (3) C (s) + O2 (g) => CO2 (g) (4) H2 (g) + O2 (g) => H2O (l) A. Formulate a methane fire reaction (CH4) according to the given reactions, note that not all reactions are balanced and unnecessary Use all responses. B. What is the theoretical amount of water you will get from...
(2) ( 2 points ) Compute AH for the reaction, 2 CH4 + C2H4(9) + 2 H2(g) given the following data: H2(g) + } 02(g) + H20(1) AH° = -285.8 kJ CO2(g) + 2 H2O(l) + CH4(g) + 2 029) AH° = 890.3 kJ 2 C2H6(g) + 7 02(g) + 4CO2(g) + 6 H2O(1) AH° = -3120.8 kJ C2H4(9) + H2(g) → C2H6(9) AH° = -136.3 kJ
equilibrium help!! What is the equilibrium constant for the reaction CO(g) + 3 H2(g) - CH4(g) + H2O(g) if at 20 °C the equilibrium molar concentrations are [CO] -0.613, [H2] = 1.839, (CH4) = 0.387, and [H20) - 0.387? Format Β Ι Ο The reaction for the formation of the diamine-silver ion is as follows: Ag (aq) + 2NH3(aq) + Ag(NH3)2(aq) a. Write the equilibrium constant expression for this reaction. for the above b. An experiment was carried out to...
Solve these two questions plz ASAP 6. Consider the chemical equation and equilibrium constant for the synthesis of ammonia at 25 °C: Ng(g) + 3 H2(g-2NH3(g) K=3.7 x 108 Calculate the equilibrium constant for the following reaction at 25 C: 7. Given the equilibrium constants for the first and second reactions, calculate the equilibrium constant for CO2 (g) + H2(g) CH3OH(g) the third reaction. K, = 1.00× 105 co(g) + H2O(g) 2co(g) + H2(g) K2 3.74x 103