For the equilibrium: 2F, (g) + O2 (g) + 600 kJ - 20F, (g) where ke= 350%3DIf the equilibrium [F2] = 2 M, [02] = 1 M, then [OF,] at equilibrium should be:700 M1400 M350 M26.5 M37.5 M

Answered: Image /qna-images/answer/14723085-166f-46ca-91dc-72e87e8745f3.jpg

Answered: For the equilibrium: 2F2 (g) + O2 (g) +…

For the equilibrium: 2F2 (g) + O2 (g) + 600 kJ = 20F2 (g) where ke= 350 If the equilibrium [F2] = 2 M, [02] = 1 M, then [OF,] at equilibrium should be: 700 M 1400 M 350 M 26.5 M 37.5 M

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

physical chem
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
Consider the following system at equilibrium where Kc = 154 and H° = -16.1 kJ/mol at 298 K. 2 NO (g) + Br2 (g) 2 NOBr (g) The production of NOBr (g) is favored by:Indicate True (T) or False (F) for each of the following: ___decreasing the temperature. ___decreasing the pressure (by changing the volume). ___decreasing the volume. ___removing NOBr . ___adding Br2 .
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?
At - 19.4 °C the pressure equilibrium constant K = 6.3 x 10' for a certain reaction. Here are some facts about the reaction: • The net change in moles of gases is -1. If the reaction is run at constant pressure, the volume increases by 12.%. If the reaction is run at constant pressure, 138. kJ/mol of heat are released. ○ Yes. Using these facts, can you calculate K, at -26. °C? ○ No. If you said yes, then enter your answer at right. Round it to 2 significant digits. at If you said no, can you at least decide whether K -26. °C will be bigger or smaller than K,, at -19.4 °C? 0 Yes, and K,, will be bigger. Yes, and K, will be smaller. ○ No. X
A] HgS occurs in two crystalline forms called "red" and "black". For the conversion of 8. L- the red form to the black form at 525 °C, 4Gº = -0.157 kJ mol-¹ and AH = 4.184 kJ mol-¹. Assuming the AH is temperature independent, find the temperature at which the two forms can coexist at equilibrium at 1.000 bar. Which is more stable above this temperature?
When 1.00 mol of H2O and 1.00 mol of CO are introduced into an empty 1.00 L container at 960 K and allowed to come to equilibrium, the mixture contains 0.422 mol of water vapor. Write the equilibrium expression for the reaction and calculate the value of Kc
Consider the following system at equilibrium where Ho = 18.8 kJ, and Kc = 9.52E-2, at 350 K: CH4(g) + CCl4(g) 2 CH2Cl2(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: whats the value of Kc The value of Q The reaction must
For a particular reaction △H= -32 kJ and △S = -98J/K (A) At what temp will the reaction be at equilibrium ? (B) If the temperature is increased from the equilibrium temperature what will happen?
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 equilibrium: 2NO, (g)–N,04 (8) AGº= – = - 5.4 kJ Now suppose a reaction vessel is filled with 5.06 atm of dinitrogen tetroxide (N,0) at 400. °C. Answer the following questions about this system: 2 rise Under these conditions, will the pressure of N,0, tend to rise or fall? 2 4 fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,0, will tend to rise, can yes that be changed to a tendency to fall by adding NO,? Similarly, if you no said the pres of N,0, will tend to fall, can that be changed to a 2 4 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.