Write the equilibrium constant for the following reaction: 2Cl2 + 2H2O <---> 4HCL + O2

Write the equilibrium constant for the following reaction:

2Cl2 + 2H2O <---> 4HCL + O2

Expert Solution

Based on the physical states of reactants and products the Kc is written. If the reactant or product are in solid or in liquid state they are represented in the expression of equilibrium constant.

queen_honey_blossom answered 3 years ago

For the reaction 4HCl(g) + O2(g)2H2O(g) + 2Cl2(g) H° = -114.4 kJ and S° = -128.9...

For the reaction 4HCl(g) + O2(g)2H2O(g) + 2Cl2(g) H° = -114.4 kJ and S° = -128.9 J/K The maximum amount of work that could be done when 2.05 moles of HCl(g) react at 308 K, 1 atm is kJ. Assume that H° and S° are independent of temperature.

Consider the reaction between HCl and O2: 4HCl(g)+O2(g)→2H2O(l)+2Cl2(g) When 63.1 g of HCl are allowed to...

Consider the reaction between HCl and O2: 4HCl(g)+O2(g)→2H2O(l)+2Cl2(g) When 63.1 g of HCl are allowed to react with 17.2 g of O2, 53.8 g of Cl2 are collected. Determine the theoretical yield of Cl2 and the percent yield for the reaction.

4HCl(g) +O2(g) >>>> 2H2O(l) + 2Cl2(g) When 63.1g of HCl are allowed to react with 17.2g...

4HCl(g) +O2(g) >>>> 2H2O(l) + 2Cl2(g) When 63.1g of HCl are allowed to react with 17.2g of O2 41.5g of Cl2 are collected A.) determine the theoretical yield of Cl2 for the reaction B.) determine the precent yield for the reaction

Given the following balanced chemical reaction: MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O(g) If 17.4...

Given the following balanced chemical reaction: MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O(g) If 17.4 g of MnO2 is reacted with 18.4g of HCl how many g of Cl2 can theoretically be produced? a. 14 g b. 144.7 g c. 75.7 g d. 8.95 g

The equilibrium constant for the reaction CCl4(g) = C(s) + 2Cl2(g) at 700ºC is 0.85. Determine the...

The equilibrium constant for the reaction CCl4(g) = C(s) + 2Cl2(g) at 700ºC is 0.85. Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 2.30 atm at 700ºC.

Part A - At 100oC, The equilibrium constant for the reaction: CF4(g) + 2H2O(g) ⇌CO2(g) +...

Part A - At 100oC, The equilibrium constant for the reaction: CF4(g) + 2H2O(g) ⇌CO2(g) + 4HF(g) is Kc,1 = 5.9 And the equilibrium constant at 100oC for the reaction: CO(g) + ½ O2(g) ⇌ CO2(g) is Kc,2 = 1.3 Compute the equilibrium constant at 100oC for the reaction (2 sig figs) 2 CF4(g) + 4H2O(g) ⇌2CO(g) + 8HF(g) + O2(g) is Kc,3 = ? Part B - Consider the reaction below (Equilibrium Constant @ 300K = Kp = 0.150)...

Calcualte the equilibrium constant for the reaction using tabulated data and write the equilibrium constant for...

Calcualte the equilibrium constant for the reaction using tabulated data and write the equilibrium constant for this reaction in terms of partial pressure 2H2(g)+O2(g) <--> 2H2O(g) at 298k, 1 bar

Write the principal equilibrium reaction and calculate the equilibrium constant for the base hydrolysis reaction of...

Write the principal equilibrium reaction and calculate the equilibrium constant for the base hydrolysis reaction of solid calcium phosphate to form monohydrogenphosphate anion as the principal phosphate containing species. Determine the pH of the solution. Ksp = 1.2 x 10-26. For H3PO4, Ka1, Ka2, and Ka3 = 7.5 x10-3 , 6.2 x 10-8 , and 4.8 x 10-13)

Q1)Determine the equilibrium constant for the following reaction at 498 K. 2 Hg(g) + O2(g) →...

Q1)Determine the equilibrium constant for the following reaction at 498 K. 2 Hg(g) + O2(g) → 2 HgO(s) ΔH° = -304.2 kJ; ΔS° = -414.2 J/K a)1.87 × 1010 b)2.31 × 10-22 c)4.33 × 1021 d)8.10 × 1031 e)5.34 × 10-11 Q2) Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° = -158 kJ; ΔS°= -219.9 J/K a)2.51 × 10-13 b)3.99 × 1012 c)3.26 × 10-12 d)13.0 e)3.07 × 1011

The reaction 2H2O2(aq)→2H2O(l)+O2(g)is first order in H2O2 and under certain conditions has a rate constant of...

The reaction 2H2O2(aq)→2H2O(l)+O2(g)is first order in H2O2 and under certain conditions has a rate constant of 0.00752 s−1 at 20.0 ∘C. A reaction vessel initially contains 150.0 mL of 30.0% H2O2 by mass solution (the density of the solution is 1.11 g/mL). The gaseous oxygen is collected over water at 20.0 ∘C as it forms. What volume of O2 will form in 80.9 seconds at a barometric pressure of 771.4 mmHg ? (The vapor pressure of water at this temperature...

Question