Use the following information to answer the next 4 questions. An equilibrium system was established in a 1.00 L flask at a certain temperature as represented by the following equation ICI(g) + Cl₂(g) ICI(g) + energy brown yellow-green bright yellow At equilibrium the flask contained 0.0571 mol of ICI(g), 1.07 mol of Cl₂(g), 1.87 mol of ICl3(g) The value of the equilibrium constant for this system is 30.6 Record your 3-digit answer

Use the following information to answer the next 4 questions. An equilibrium system was established in a 1.00 L flask at a certain temperature as represented by the following equation ICI(g) + Cl₂(g) ICI(g) + energy brown yellow-green bright yellow At equilibrium the flask contained 0.0571 mol of ICI(g), 1.07 mol of Cl₂(g), 1.87 mol of ICl3(g) The value of the equilibrium constant for this system is 30.6 Record your 3-digit answer

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 10 Which one of the following statements does not describe the equilibrium state? O Equilibrium is dynamic and both forward and reverse reactions never stop. O The concentration of the reactants is equal to the concentration of the products. O The concentration of the reactants and products reach a constant level. O The rate of the forward reaction is equal to the rate of the reverse reaction.
Hydrogen and iodine react to form hydrogen iodide, like this: H₂(g) + I₂(g) → 2 HI(g) Use this chemical equation to answer the questions in the table below. Suppose 220. mmol of H₂ and 220. mmol of I₂ are added to an empty flask. How much HI will be in the flask at equilibrium? Suppose 175. mmol of HI are added to an empty flask. How much HI will be in the flask at equilibrium? None. Some, but less than 440. mmol. 440. mmol. More than 440. mmol. None. Some, but less than 175. mmol. O 175. mmol. More than 175. mmol. X Ś
QUESTION 25 Consider the following reversible reaction at equilibrium: 3 H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the reactants (left side)? O Decreasing the temperature. O Increasing the amount of H2. O Adding a catalyst to the system. O Decreasing the volume of the system. O Increasing the amount of NH3.
Indicate whether the sentence or statement is true Tor false F. If false, change the word or phrase in bold italics to make the sentence or statement true by writing the correct word or phrase in the space provided. At equilibrium, the forward and reverse reactions are happening at the same rate. The following reaction is an example of heterogeneous equilibrium. 2NH3(g) N₂ + 3H₂(g) In the graph below, equilibrium has been reached when all the lines have leveled off. CONCENTRATION (mol/L) TIME (min) For the gaseous equilibrium shn, 3A + B 4C+D+ heat, adding heat to the reaction will cause the reaction to shift to the right. For the gaseous equilibrium the quantity of A will incre N₂ M₂ Ny The equilibrium law express K = [H₂HIN INH own, 3. + B 4C + D + heat. If substance D is added to the system, e 3X as much as the quantity of B n for the following reaction 2NH3(g) N₂(g) + 3H₂(g) is The equilibrium law expres in for the reaction Mg) + 2AgNO3(aq) is Ke= [Mg(NO3)2 [AgNO3(aq) 2Ag) +…
Question 16 In the equilibrium reaction, N₂(g) + 3H₂(g) → 2NH3(g) the production of ammonia is the endothermic reaction. When the equilibrium system is heated, the production of ammonia will A increase decrease not be affected B C OA B OC
Consider the following system at equilibrium: CH4(g) + 2H20(g) CO2(g) + 4H2(g) What change will cause the equilibrium to shift to form more CH4? Multiple Choice decrease (H2] increase (H20] decrease the volume of the reaction vessel increase (CH4] decrease [CO2] DELL
Consider this equilibrium 4HC1(g) + O₂(g) 2H₂O(g) + 2Cl (g) The equilibrium law expression for the balanced chemical equation would be [HC][0₂]/[H₂O][C1₂] Option 1 2[H₂0][C1₂]/ 4[HC1][0₂] Option 3 [H₂0][C1₂]/HC1][0₂] Option 5 [H₂OF[C1₂ [HCI][0₂] Option 2 [HCI][0₂]/[H₂O1[C1₂F Option 4
When the temperature of a system in equilibrium is decreased, what will happen to equilibrium? shifts towards absorbing heat reduces the number of moles increases the number of moles Shift towards releasing heat
The equilibrium system between sulfur dioxide gas, oxygen gas, and sulfur trioxide gas is given. 2SO2(g)+O2(g)↽−−⇀ 2SO3(g)2SO2(g)+O2(g)↽−−⇀ 2SO3(g) Write the balanced chemical equation for the reverse reaction. Include physical states for all species.
For questions 9-13. Consider the reaction 2NOCI(g) = 2NO(g) + C12(g). If this reaction is at equilibrium, what happens when the following changes occur? 9. NOCI(g) is added O shift to right shift to left no reaction O both shifts to right and left
System at equilibrium before temperature is increased. Consider the reaction, A =B AH = -45 kcal/mol (A = white spheres and B = black spheres) Identify the new equilibrium scenario after a temperature increase. Select the new equilbrium scenario:
Use the following reaction to answer the questions below. N2 (9) + 3 H2 (g) → 2 NH3 (9) + heat Increasing the temperature of the reaction would cause the equilibrium to shift in which direction? Towards the products Towards the reactants No shift would occur Cannot be determined with the given information Increasing the amount of hydrogen in the reaction would cause the equilibrium to shift in which direction? Towards the products Towards the reactants No shift would occur Cannot be determined with the given information