2 H2O (g) + 2 Cl2 (g) + heat ----------> 4 HCl (g) + O2 (g)...

2 H2O (g) + 2 Cl2 (g) + heat ----------> 4 HCl (g) + O2 (g) 3. Which of the following is true about reaction when O2 (g) is added to the mixture. a. Equilibrium will shift to the left. b. Equilibrium will shift to the right. c. No effect on the equilibrium. d. Equilibrium constant will decrease. 4. Which of the following is true about reaction when the pressure is increased by the addition of an inert gas? a. Equilibrium will shift to the left. b. Equilibrium will shift to the right. c. No effect on the equilibrium. d. Equilibrium constant will decrease. 5. Which of the following is true about reaction when the size of the reaction container is increased? a. Equilibrium will shift to the left. b. Equilibrium will shift to the right. c. No effect on the equilibrium. d. Equilibrium constant will increase.

Expert Solution

2 H2O (g) + 2 Cl2 (g) + heat ----------> 4 HCl (g) + O2 (g)

1. Addition of O2 means we are adding products . Addition of products increases the rate of back ward reaction . so equilibrium shift to left ie towards reactionts side. answer is a. Equilibrium will shift to the left.

2. Increasing presure favours the equilibrium towards the less number of moles side.. Reactants have less number of moles than products. equilibrium shift to left ie towards reactants side.

answer is a. Equilibrium will shift to the left.

3. Increasing size of container means increasing volume of the reaction.

increasing volume of the reaction favours towards more number of moles side. producs have more number of moles than reactants.

equilibrium shift to right side ie towards product side .

answer b. Equilibrium will shift to the right.

queen_honey_blossom answered 2 years ago

heat of reaction at 400c for the following reaction: HCl(g) + O2= Cl2(g) + H2O (g)...

heat of reaction at 400c for the following reaction: HCl(g) + O2= Cl2(g) + H2O (g) HHV and LHV for liquid acetone (in KJ/Kg)

2C2H2 (g) + 5 O2 (g) ---------> 4 CO2 (g) + 2 H2O (g) + heat...

2C2H2 (g) + 5 O2 (g) ---------> 4 CO2 (g) + 2 H2O (g) + heat 3. Which of the following is true about reaction when the concentration of O2 (g) is decreased? a. Equilibrium will shift to the left. b. Equilibrium will shift to the right. c. No effect on the equilibrium. d. Equilibrium constant will decrease. 4. Which of the following is true about reaction when the temperature is increased? a. Equilibrium will shift to the left. b....

Consider the combustion of hydrochloric acid. 4 HCl (aq) + O2(g)  2H2O(l) + 2 Cl2(g)...

Consider the combustion of hydrochloric acid. 4 HCl (aq) + O2(g)  2H2O(l) + 2 Cl2(g) ΔHrxn = + 96.976 kJ/mol B.If you place 750 mL of 0.500 M solution of HCl with 17.2 g of O2, will any oxygen remain? (Hint: limiting reagent problem) C.What mass of chlorine gas (in grams) is produced? D) How many molecules of Cl2 are produced based on part (B) E) What mass of excess reagent remains after the limiting reagent is used up?...

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O ∆Hrxn = -906 kJ A)...

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O ∆Hrxn = -906 kJ A) Calculate the heat (in kJ) associated with the complete reaction of 0.127 Kg of NH3. B) What mass of O2 (g) is required to evolve 4605 kJ of energy

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) A scientist adds 7.00 atm...

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) A scientist adds 7.00 atm of NH3(g) and 8.00 atm of O2(g) to a 5.0 L container at 473 K. What will the pressure of H2O(g) be if the reaction goes to completion? Assume that the temperature remains constant. Select one: a. 6.40 atm b. 9.60 atm c. 10.5 atm d. 0.90 atm e. 15.0 atm

CH4(g) + Cl2(g)  CH2Cl2(g) + 2 HCl(g) Use the data in the table below to...

CH4(g) + Cl2(g)  CH2Cl2(g) + 2 HCl(g) Use the data in the table below to calculate the standard enthalpy, ∆H˚, for the reaction above. Substance CH4(g) CH2Cl2(g) HCl(g) ∆Hf˚, kJ•mol-1 –74.6 –95.4 –92.3

Consider the following chemical reaction: 2 CH4(g) 3 O2(g) 2 CO(g) 4 H2O(l) Select all the...

Consider the following chemical reaction: 2 CH4(g) 3 O2(g) 2 CO(g) 4 H2O(l) Select all the statements that are correct: The reaction should become more product favored at high temperatures The reaction should become more product favored at low temperatures The reactants can adopt a larger number of configurations than the products The potential energy of the reactants is higher than the potential energy of the products The potential energy of the reactants is lower than the potential energy of...

Given the following balanced reaction, O2(g) + 4 H+(aq) + 4 Fe2+(aq) → 2 H2O(l) +...

Given the following balanced reaction, O2(g) + 4 H+(aq) + 4 Fe2+(aq) → 2 H2O(l) + 4 Fe3+(aq) What is the equilibrium constant (K)? The following information may be useful. O2(g) + 4 H+(aq) + 4e- → 2 H2O(l) Eº = 1.23 V Fe3+(aq) + e- → Fe2+(aq) Eº = 0.77 V

2) Consider the equation: CHCl3(g) + Cl2(g)  CCl4(g) + HCl(g) The initial rate of reaction...

2) Consider the equation: CHCl3(g) + Cl2(g)  CCl4(g) + HCl(g) The initial rate of reaction is measured at several different concentrations of the reactants with the following results From the data, determine: a. the rate law for the reaction b. the rate constant (k) for the reaction CHCl3 Cl2 rate M/s 0.125 M 0.100 M 0.0025 M/s 0.250 M 0.100 M 0.0100 M/s 0.250 M 0.200 M 0.0200 M/s

In the Deacon process for the manufacture of chlorine, HCl and O2 react to form Cl2...

In the Deacon process for the manufacture of chlorine, HCl and O2 react to form Cl2 and H2O. Sufficient air (21 mole % O2, 79% N2) is fed to provide 35.0% excess oxygen and the fractional conversion of HCl is 75.0%. a. Calculate the mole fractions of the product stream components using atomic species balances in your calculation. b. Again calculate the mole fractions of the product stream components using the extent of reaction and stoichiometric coefficients in the calculation...

Question