CH 4(g) 2(g) H2CO 9 DH = - 135.2 Kcal Consider the following system at equilibrium: Complete the following table. Indicate changes in moles and concentrations by entering I, D, N, or ? in the table. (I = increase,D decrease, N = no change, ? = insufficient information to determine) Change in number of moles Change in molar Direction of shift, left, right or no change to re-establish, equilibrium (After stress has been imposed) concentration Chq Change or stress imposed on the system at equilibrium |02 CH4 C02 H2CO CH4 H2CO AH

CH 4(g) 2(g) H2CO 9 DH = - 135.2 Kcal Consider the following system at equilibrium: Complete the following table. Indicate changes in moles and concentrations by entering I, D, N, or ? in the table. (I = increase,D decrease, N = no change, ? = insufficient information to determine) Change in number of moles Change in molar Direction of shift, left, right or no change to re-establish, equilibrium (After stress has been imposed) concentration Chq Change or stress imposed on the system at equilibrium |02 CH4 C02 H2CO CH4 H2CO AH

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter17: Equilibrium

Section: Chapter Questions

Problem 72A

See similar textbooks

Similar questions

For the following reactions, predict whether the pressure of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. (a) H2O(l)H2O(g) (b) N2(g)+3H2(g)2NH3(g) (c) C2H4(g)+H2O(g)C2H5OH(g)
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
The following data apply to the unbalanced equation A(g)B(g) (a) On the basis of the data, balance the equation (simplest whole-number coefficients). (b) Has the system reached equilibrium? Explain.
Which direction of the equilibrium 2NO2(g)N2O4(g)+59.0kJ will be favored if the system is cooled? Explain.
Mustard gas, used in chemical warfare in World War I, has been found to be an effective agent in the chemotherapy of Hodgkin's disease. It can be produced according to the following reaction: SCl2(g)+2C2H4(g)S(CH2CH2Cl)2(g)An evacuated 5.0-1- flask at 20.0C is filled with 0.258 mol SCl2 and 0.592 mol C2H4. After equilibrium is established, 0.0349 mol mustard gas is present. (a) What is the partial pressure of each gas at equilibrium? (b) What is K at 20.0C?
In the following equilibrium in a closed system, indicate how the equilibrium is shifted by the indicated stress: HF(g)+H2O(l)H3O+(aq)+F(aq) (a) Additional HF(g) is added to the system. (b) Water is added. (c) Ca( NO3)2 solution is added, and CaF2 precipitates. (d) The volume is reduced. (e) KOH is added. (f) A catalyst is added.
If a reaction is reversible, when can it be said to have reached equilibrium?
Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)
The following is a thought experiment. Imagine that you put a little water in a test tube and add some NaF crystals. Immediately after you add NaF, you observe that the crystals begin dissolving. The quantity of solid NaF decreases, hut before long, it appears that no more NaF is dissolving. The solution is saturated. The equation for the dissolution of NaF in water is NaF(s) —* Na (aq) + F~(aq). As NaF dissolves, what do you think happens to the rate of dissolution? Describe w hat is occurring on the molecular level. Assume that the reverse reaction, Na+(aq) + F“(aq) —* NaF(s), also occurs as the crystal dissolves. In other words, both dissolution and precipitation are taking place. When it appears that there is no more change in the quantin’ of NaF dissolving (the solution is saturated), w hat has happened to the rates of the forward and reverse reactions? Explain your answer.
5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?