The equilibrium reaction Fe; O4(s) + 3 H2(g) 2 3 Fe(s) +4 H2O(g) has AH° = 149,77 kJ /mol. Write down Shift Left, Shift Right, or No Change for each of the following situations: a) Solid Fe is added to the reaction. b) The temperature of the reaction is increased. c) The volume of the reaction vessel is suddenly doubled with no change in temperature. d) After doubling the volume of the reaction vessel, the partial pressure of H20 is tripled with no change in temperature.

The equilibrium reaction Fe; O4(s) + 3 H2(g) 2 3 Fe(s) +4 H2O(g) has AH° = 149,77 kJ /mol. Write down Shift Left, Shift Right, or No Change for each of the following situations: a) Solid Fe is added to the reaction. b) The temperature of the reaction is increased. c) The volume of the reaction vessel is suddenly doubled with no change in temperature. d) After doubling the volume of the reaction vessel, the partial pressure of H20 is tripled with no change in temperature.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

For the reaction NO₂(g) + SO₂(g) →→ NO(g) + SO3(g), AH° = -41.8 kJ. How will the equilibrium concentration of NO be affected if: NO2 is removed from the container. O Concentration stays the same. O Concentration decreases. O Concentration increases. SO3 is added to the container. O Concentration increases. O Concentration stays the same. O Concentration decreases. The temperature of the reaction mixture is raised. O Concentration increases. O Concentration stays the same. O Concentration decreases. SO₂ is removed from the container. O Concentration stays the same. Concentration decreased. O Concentration increased. The pressure of the gas mixture is raised by compressing the volume to 3.00 L. O Concentration decreases. O Concentration stays the same. O Concentration increases.
Consider the following reaction at equilibrium. What effect will doubling the temperature have on the system? CH4 ( + 2 02 () = CO2 (g) + 2 H2O () AH° = -882.0 kJ O No shift will occur because the volume of the system has not changed. No shift will occur because the total number of gas molecules on both sides of the chemical equation are equal. O A shift left towards reactants will occur. O No shift will occur because none of the concentrations have changed. O A shift right towards products will occur.
3.) For the following equilibrium reaction2NO2(g) ↔N2O4(g) + Δlook in the Tro text to see what LeChatelier's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. [Hint: remember that PV=nRT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.
Consider the following equilibrium: 2NOC1 (g) → 2NO(g) + Cl₂ (g) AG = 41. kJ Now suppose a reaction vessel is filled with 8.30 atm of nitrosyl chloride (NOC1) and 5.80 atm of chlorine (C1₂) at 878. °C. Answer the following questions about this system: Under these conditions, will the pressure of Cl₂ tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of Cl₂ will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. оо rise fall yes no 0 atm x10 X Ś
Methane and water react to form carbon monoxide and hydrogen, like this: CH2(g)+H₂O(g) CO(g)+3H2(g) Suppose a mixture of CH 4, H2O, CO and H2 has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium to the right The pressure of CH4 will ? to the left Some CO is added. The pressure of H2O will ? (none) to the right The pressure of H2O will ? Some CH4 is removed. to the left The pressure of CO will ? (none)
Nitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no change
Methane and water react to form hydrogen and carbon monoxide, like this: CH4(g) + H₂O(g) → 3 H₂(g) + CO(g) The reaction is endothermic. Suppose a mixture of CH4, H₂O, H₂ and CO has come to equilibrium in a closed reaction vessel. Predict what change, if perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. any, the perturbation change in composition The temperature is raised. The pressure of CH4 will The temperature is lowered. The pressure of H₂ will ? ? ↑ î shift in equilibrium O X to the right to the left (none) to the right to the left (none) Ś
Consider the following equilibrium: 2NH3(g) = N₂ (g) + 3H₂(g) 2 AG = 34. kJ Now suppose a reaction vessel is filled with 7.87 atm of ammonia (NH3) and 1.17 atm of hydrogen (H₂) at 448. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise fall yes no atm x10 X 5
When heated, carbon monoxide reacts with water to produce carbon dioxide and hydrogen. CO(g) + H2O(g) <--> CO2(g) + H2(g) +heat For each of the following changes at equilibrium, indicate whether the equilbrium shifts in the directions of the products, the reactants, or does not change: (a) decreasing the temperature (b) adding more H2(g) (c) removing some CO2(g) (d) adding more H2O(g) (e) decreasing the volume of the container
Consider the reaction: CH4(g) + H2O(g) ⇌ CO(g) + 3H2(g); DHo = 206 kJ (D = delta) Which of the following changes will increase the concentration of hydrogen gas at equilibrium and the value of K? (A) Increasing the reaction temperature; (B) Adding more CO(g) to the reaction mixture while maintaining a constant temperature; (C) Adding more CH4 and H2O(g) while maintaining a constant temperature; (D) Increasing the pressure of the reaction mixture while maintaining a constant temperature.
Consider the following equilibrium: N₂ (g) + 3H₂(g) → 2NH3(g) AG = -34. KJ Now suppose a reaction vessel is filled with 3.40 atm of nitrogen (N₂) and 4.50 atm of ammonia (NH3) at 250. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to 2 significant digits. OO rise fall yes no atm ☐x10 X Ś
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2( g) + Cl2( g)Δ2 ICl( g) Kp = 81.9 (at 298 K) A reaction mixture at 298 K initially contains PI2 = 0.25 atm and PCl2 = 0.25 atm. What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?a) 0.17 atm b) 0.64 atmc) 0.41 atm d) 2.3 atm