If you were a chemist and trying to maximize the amount of decomposition of CIF, which of the following tactics might you try? Assume that the mixture reaches equilibrium. Check all that apply. O add a catalyst to increase the rate of decomposition O remove F, from the reaction miocture as it forms. O increase the reaction temperature O increase the volume of the reaction container

If you were a chemist and trying to maximize the amount of decomposition of CIF, which of the following tactics might you try? Assume that the mixture reaches equilibrium. Check all that apply. O add a catalyst to increase the rate of decomposition O remove F, from the reaction miocture as it forms. O increase the reaction temperature O increase the volume of the reaction container

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

Question 16 If the reaction quotient, Q, is less than Kin an equilibrium reaction, then O a. the chemical system has reached equilibrium. O b. the reaction will proceed in the backward direction until equilibrium is established. Oc. the reaction will proceed in the forward direction until equilibrium is established. O d. the temperature must be increased for the reaction to proceed in the forward direction. e. the reaction will proceed in the direction that increases the number of mole of substances.
Suppose a 500. mL flask is filled with 0.80 mol of NO, and 1.8 mol of NO,. The following reaction becomes possible: NO,(g) + NO(g) - 2NO,(g) The equilibrium constant K for this reaction is 4.18 at the te perature of the flask. Calculate the equilibrium molarity of NO,. Round your answer to two decimal places. Fducation AR Rights Re
When considering the reaction at equilibrium which direction will the reaction shift (left, right, no effect) to compensate for the following permutations? 1. Adding more HNO3. 2. Siphoning off the N2. 3. Decreasing the temperature of the system. 4. Increasing the pressure of the system.
Equilibrium is reached in a chemical reaction when A. the reactants are completely consumed. B. the concentrations of all reactants and products become equal. C. the rates of the opposing reactions become equal. D. the forward and reverse reactions stop.
Chemical or physical processes that can proceed in both the forward and reverse directions are called reversible processes redox processes O combustion processes equilibrium processes Next • Previous
4. Name two ways in which a system at equilibrium can be disturbed.
QUESTION 19 Consider the following information, choose all of the statements that are false. k] H2(g) + S(s) = H,S(g) K=7.8x105 AH= -20.17 mol O Adding a catalyst will cause the concentration of H25 to increase. O Decreasing the volume of the reaction vessel will cause the concentration of H2 to increase. O Products are predominant. OIncreasing the reaction temperature will cause the concentration of H2 to increase. O Adding more H25 will cause the concentration of H2 to decrease. O Removing S will cause the concentration of H2 to increase.
Which of the following is TRUE regarding chemical reactions at equilibrium? Select one: O a. The reaction will proceed spontaneously O b. No further concentration changes between reactants and products take place O c. The reactant and product concentrations are equal O d. None of the following are true
4. What does a bi-directional arrow tell you about a chemical reaction? The reaction happens only once The reaction happens more than once The reaction is able to reverse O The reaction is at equilibrium
What approximation can be made when the equilibrium constant is very small in order to simplify the math involved with an equilibrium problem? O a) Assume the concentration of each product equals zero. b) Assume this problem cannot be solved by mere humans. c) Assume the reactant concentrations go to zero. d) Assume that the reactant concentrations do not change significantly.
What effect, if any, would increasing the pressure have on the equilibrium?
At constant temperature, reducing the volume of a gaseous equilibrium mixture causes the reaction to shift in the direction that increas of moles of gas in the system.