Consider the following equilibrium: 2NO (g) + Cl, (g) 2NOCI (g) AG°- -41. kJ Now suppose a reaction vessel is filled with 2.44 atm of chlorine (Cl,) and 9.81 atm of nitrosyl chloride (NOCI) at 491. °C. Answer the following questions about this system: O rise Under these conditions, will the pressure of NOCI tend to rise or fall? O fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOCI will tend to rise, can that O yes be changed to a tendency to fall by adding NO? Similarly, if you said the O no pressure of NOCI 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. atm Round your answer to 2 significant digits.

Consider the following equilibrium: 2NO (g) + Cl, (g) 2NOCI (g) AG°- -41. kJ Now suppose a reaction vessel is filled with 2.44 atm of chlorine (Cl,) and 9.81 atm of nitrosyl chloride (NOCI) at 491. °C. Answer the following questions about this system: O rise Under these conditions, will the pressure of NOCI tend to rise or fall? O fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOCI will tend to rise, can that O yes be changed to a tendency to fall by adding NO? Similarly, if you said the O no pressure of NOCI 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. atm Round your answer to 2 significant digits.

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

Consider the following equilibrium: 2NH₂ (g)-N₂ (g) + 3H₂(g) AG-34. KJ Now suppose a reaction vessel is filled with 4.85 atm of ammonia (NH3) a system: Under these conditions, will the pressure of H, tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of H, will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of H₂ 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. and 2.40 atm of hydrogen (H₂) at 658. °C. Answer the following questions about this Ⓒrise O fall yes no atm 10 10 X S
Choose the letter of the correct answer. N204 (g) = (reversible to) 2NO2 (g), K = 4.63 x 10-3 I. the given is equation is an example of homogenous equilibrium II. Equilibrium will lie to the right Which statement(s) is/are correct?
Explain thoroughly and answer
Consider the following equilibrium: N₂(g) + 3H₂(g)2NH, (g) AG- --34, k Now suppose a reaction vessel is filled with 2.94 atm of nitrogen (N₂) and 1.53 atm of ammonia (NH₂) at 239. "C. Answer the following questions about this system: Under these conditions, will the pressure of NH, 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 NH, 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. Orise O fall O yes O no
The oxidation of ammonia into nitric oxide is an exothermic process. AH n = -904.4 kJ INO) + 6H,0(g) equilibrium of the system? 4NH,(g) + 5O,(g) How will the following conditions affecs the Adding more O, a. b. Adding H,O Removing NH, с. d. Increasing the temperature of the system Decreasing the pressure in the vessel e.
Consider the following system at equilibrium: N2(g) + 3H2(g) 2NH3(g) + 92.94 kJWhich of the following changes will shift the equilibrium to the right? I. increasing the temperature II. decreasing the temperature III. increasing the volume IV. decreasing the volume V. removing some NH3 VI. adding some NH3 VII. removing some N2 VIII. adding some N2 Group of answer choices I, IV, VI, VII II, III, V, VIII I, VI, VIII I, III, V, VII II, IV, V, VIII
Consider the following reaction that takes place at 1200 °C: H, (g) + CI, (g) + 2HCI (g) Kc = 2.5x10 Hydrogen gas and chlorine gas were added to a reaction vessel at partial temperatures of 2.00 atm and 1.00 atm, respectively. Calculate the total pressure in the flask at equilibrium.
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
Consider the following reaction:2NOBr(g) 2NO(g) + Br2(g) If 0.224 moles of NOBr, 0.330 moles of NO, and 0.384 moles of Br2 are at equilibrium in a 14.0 L container at 518 K, the value of the equilibrium constant, Kp, is .
Heating HI(g) at 425 °C causes some of this compound to decompose, forming H2 (g) and I2 (g). Eventually, the amounts of the three species do not change further, the system has reached equilibrium. (At this point, approximately 22% of the HI has decomposed.) What is happening in this system at the molecular level? O H2(g) reacts with I2 (g) to produce HI(g) at the same rate as it decomposes. H2 (g) and I2 (g) molecules collide with HI(g) making the reaction stop. Only part of the HI(g) molecules has enough energy to decompose at this temperature. 5:55 PM FLV 2/22/2020 Type here to search hp ins prt sc delete home f12 f8 f9 f10 f5 f6 f7 14 10 num & backspace lock 23 8. 3 %24
Consider the following equilibrium: N₂(g) + 3H₂(g) 2NH, (g) AG=-34. kl Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 8.20 atm of ammonia (NH,) at 814. "C. Answer the following questions about this system: Under these conditions, will the pressure of H₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂¹ In other words, If you said the pressure of H₂ will tend to rise, can that be changed to a tendency to fall by adding Ny? Similarly, if you said the pressure of Hy will tend to fall, can that be changed to a tendency to rise by adding N₂7 If you said the tendency can be reversed in the second question, calculate the minimum pressure of N, needed to reverse it. Round your answer to 2 significant digits. Orie fall O yes Ono 7 p X 5 OG F# S
Consider the following reaction:COCl2(g) CO(g) + Cl2(g)If 2.98×10-2 moles of COCl2, 0.206 moles of CO, and 0.304 moles of Cl2 are at equilibrium in a 17.8 L container at 672 K, the value of the equilibrium constant, Kp, is .