Calculate Kc for the following reaction: 2CH3OH(g) + H2(g) ⇌ C2H6(g) + 2H2O(g) given the following...

Calculate Kc for the following reaction: 2CH3OH(g) + H2(g) ⇌ C2H6(g) + 2H2O(g) given the following data:

2CH4(g) ⇌ C2H6(g) + H2(g) ;Kc1 = 9.4×10−13

CH4(g) + H2O(g) ⇌ CH3OH(g) + H2(g) ;Kc2 = 2.4 ×10−21

If needed, use “E” for scientific notation. Report your answer to the correct number of significant figures.

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Using the following data, calculate the Hrxnfor the reaction: C2H4(g) + H2(g) →C2H6(g) (ch8) 1.H2(g) +...

Using the following data, calculate the Hrxnfor the reaction: C2H4(g) + H2(g) →C2H6(g) (ch8) 1.H2(g) + . O2(g) H2O(ℓ)H1= –285.8 kJ 2.C2H4(g) + 3 O2(g) 2 H2O(ℓ) + 2 CO2(g)H2= –1411 kJ 3.3 H2O(ℓ) + 2 CO2(g) 7/2 O2(g) + C2H6(g)H3= –(–1560 kJ)

Kc for the following reaction is 0.35. H2 (g) + I2 (g) 2 HI (g). If...

Kc for the following reaction is 0.35. H2 (g) + I2 (g) 2 HI (g). If 1.0 mol of I2 and 1.0 mol of H2 are placed in a 1.0 L vessel, the equilibrium concentration of HI is : The answer is 0.46 M, please explain how this value was reached. Thanks!

For the following reaction: H2(g) + I2(g)<--->2HI(g) ; Kc=49.5 The beginning concentrations are: H2: 0.10M, I2:...

For the following reaction: H2(g) + I2(g)<--->2HI(g) ; Kc=49.5 The beginning concentrations are: H2: 0.10M, I2: 0.050M, and HI:0 Assume this reaction is not at equilibrium. When it does reach equilibrium, what will the concentrations be?

Consider the following reaction: H2(g) +Br2(g) <=> 2HBr(g) Kc=2.0x10^9 at 25C If 0.100 mol H2 and...

Consider the following reaction: H2(g) +Br2(g) <=> 2HBr(g) Kc=2.0x10^9 at 25C If 0.100 mol H2 and 0.200 mol of Br2 were placed in a 10.0L container at 25C, what will the equilibrium concentrations of H2, Br2 and HBr be?

The equilibrium constant Kc is 54.3 at 430°C for the following reaction: H2(g) + I2(g) ⇌...

The equilibrium constant Kc is 54.3 at 430°C for the following reaction: H2(g) + I2(g) ⇌ 2HI(g) Initially, 0.90 M H2, I2, and HI are introduced into a 5.0-L flask and allowed to come to equilibrium. What are the equilibrium concentrations of H2, I2, and HI in the flask? (10 points) (Does the size of flask matter since Molarity is given?)

1) C2H6 (g) -----> C2H4 (g) + H2 (g) ΔH1 = ? 2) C2H6 (g) +...

1) C2H6 (g) -----> C2H4 (g) + H2 (g) ΔH1 = ? 2) C2H6 (g) + 3.5O2 (g) -----> 2CO2 (g) + 3H2O (l) ΔH2 = -1558 kJ/mo 3) C2H4 (g) + 3O2 (g) -----> 2CO2 (g) + 2H2O (l) ΔH3 = -1408 kJ/mol 4) 2H2O (l) -----> 2H2 (g) + O2 (g) ΔH4 = 568 kJ/mol A: Calculate ΔHrxn for reaction (1) based on the given data. Is this reaction endothermic or exothermic? B: How much heat is transferred...

Calculate delta H for the reaction H(g) + Br(g) = HBr(g), given the following information: H2(g)...

Calculate delta H for the reaction H(g) + Br(g) = HBr(g), given the following information: H2(g) + Br2(g) = 2HBr(g) delta H = -72 kJ H2(g) = 2H(g) delta H = +436 kJ Br2(g)= 2Br(g) delta H = +224 kJ

Consider the reaction: C2H4(g) + H2(g) <-> C2H6(g). For this process, deltaH = -137.0 kj/mol and...

Consider the reaction: C2H4(g) + H2(g) <-> C2H6(g). For this process, deltaH = -137.0 kj/mol and deltaS = -120.6 J/mol*K. Based on these data and assuming deltaH and deltaS are temperature independent, answer the following questions; 1) Does this reaction favor products or reactants at 25 degrees C? 2) At 25 degrees C, is the reaction driven(dominated) by the entropy or the enthalpy? 3) Would a decrease in temperaturefavor the reactants or the products? 4) At what temperature would the...

Kc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌...

Kc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430°C. Calculate the equilibrium concentrations of H2, I2, and HI at 430°C if the initial concentrations are [H2] = [I2] = 0 M, and [HI] = 0.547 M. [H2]= [I2]= [HI]=

1. Calculate delta S at 27*c: 2CH4 (g) --> C2H6 (g)+ H2 (g) 2. Calculate delta...

1. Calculate delta S at 27*c: 2CH4 (g) --> C2H6 (g)+ H2 (g) 2. Calculate delta S at 27*c: 2NH3 (g) --> N2H4 (g) + H2 (g) 3. If delta H (+) and delta S (-) is it spontaneous?

Subjects