Consider the following equilibrium:N₂(g) + 3H₂(g) → 2NH3 (g)Now suppose a reaction vessel is filled with 7.18 atm of nitrogen (N₂) and 0.0762 atm of ammonia (NH3) at 359. °C. Answer thefollowing questions about this system:AGO== -34. kJUnder these conditions, will the pressure of NH3 tend to rise or fall?H₂?Is it possible to reverse this tendency by addingIn other words, if you said the pressure of NH3 will tend to rise, can thatbe changed to a tendency to fall by adding H₂? Similarly, if you said thepressure of NH3 will tend to fall, can that be changed to a tendency torise by adding H₂?If you said the tendency can be reversed in the second question, calculatethe minimum pressure of H₂ needed to reverse it.Round your answer to 2 significant digits.risefall0yesO noatmx10X

Given reaction is the formation reaction of Ammonia and we have to find out the direction of…

Consider the following equilibrium: N₂(g) + 3H₂(g) → → 2NH3(g) AGO = = -34. KJ Now suppose a reaction vessel is filled with 7.18 atm of nitrogen (N₂) and 0.0762 atm of ammonia (NH3) at 359. °C. Answer the ollowing questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? rise fall 0 x10

Consider the following equilibrium: N₂(g) + 3H₂(g) → → 2NH3(g) AGO = = -34. KJ Now suppose a reaction vessel is filled with 7.18 atm of nitrogen (N₂) and 0.0762 atm of ammonia (NH3) at 359. °C. Answer the ollowing questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? rise fall 0 x10

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...

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32 Consider the reaction: kJ 2SO₂(g) + O₂(g) =2SO3(g) AH= - 198.2 mol How would the concentrations of SO2, O₂, and SO3 at equilibrium change if we were to increase the temperature? Select the single best answer for each part. Part 1 of 3 [s0₂]: The concentration increases. [0₂]: The concentration decreases. There is no change. Part 2 of 3 The concentration increases. The concentration decreases. There is no change. X X S
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.
The following gases are in equilibrium in a sealed glass tube. 2 NO2 (g) = N2O4 (g) (brown) (colorless) Increasing the temperature makes the gas in the tube more intensely brown in color. Decreasing the temperature has the opposite effect. Based on this observation, the reaction shown must be... O neither exothermic nor endothermic O endothermic exothermic
following equilibrium reaction at 160.00 °C. If 0.420 atm of H2O2(g) is initially present, calculate the equilibrium partial pressures of H2(g), O2(g), and H2O2(g).
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A sample of H,S(g) at 0.495 atm is placed in a container and the following reaction reaches equilibrium. What is the total pressure of all gases in the container? 2H2S(g) = 2H2(g) + S2(g) K, = 3.85 x 10-7 0.497 atm 0.215 atm 0.793 atm 0.624 atm 0.387 atm O O O
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 hydrogen (H₂) and 9.24 atm of ammonia 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 O fall yes Ono X (NH3) at 736. °C. Answer the following questions about this S
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A reaction vessel initially contains 6.30 atm of A and 2.10 atm of B. A reaction occurs according to the equation:2A(g)+B(g)⇆2C(g)2A(g)+B(g)⇆2C(g)When equilibrium is reached, the total pressure is found to be 6.51 atm. What is the equilibrium constant Kp?Please enter your response to three significant figures using decimal notation.
Consider the following equilibrium: N,0, (g) = 2NO, (3) AG' = 5.4 kJ Now suppose a reaction vessel is filled with 0.496 atm of nitrogen dioxide (NO,) at 137. °C. Answer the following questions about this system: O rise Under these conditions, will the pressure of NO, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,O,? In other words, if you said the pressure of NO, will tend to rise, can that O yes be changed to a tendency to fall by adding N,04? Similarly, if you said O no the pressure of NO, will tend to fall, can that be changed to a tendency to rise by adding N,0,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N,0, needed to reverse it. O atm Round your answer to 2 significant digits.
8. Consider the equilibrium reaction: N2(g) + O2(g) = 2 NO(g) Kp 4.10 x 10³ at 2000°C a) If 1.00 atm of nitrogen gas and 1.00 atm of oxygen gas is mixed with 0.10 atm of nitrogen monoxide in a 500.0 mL container at 2000°C, in which direction will the reaction proceed to reach equilibrium? Show all work to justify your answer. b) What is the concentration of each gas when equilibrium is reached at 2000°C? Show all your work. Equilibrium Partial Pressures: PN₂ = Po₂ = 1.02 atm and PNO = 0.07 atm Use PV = nRT Answer: Equilibrium Concentrations: [N₂] = [0₂] = 5.47 x 10-3 mol/L and [NO] = 4 x 10+ M