46 46 11:02 bD - If both statements are FALSEAn increase in pressure favors a shift in the direction that will reduce thevolume of the gas system, considering that the molecules are readilycompressible. However, a change in solution pressure will have anegligible effect on the equilibrium.A - If the first statement is TRUE and the second statement is FALSEB-If the first statement is FALSE and the second statement is TRUEC - If both statements are TRUEOD- If both statements are FALSEAn endothermic forward reaction will favor a shift to the right, allowing adecrease in the equilibrium constant. This is attributable to the release ofheat as compared to exothermic reactions.A - If the first statement is TRUE and the second statement is FALSEB-If the first statement is FALSE and the second statement is TRUEC-If both statements are TRUED - If both statements are FALSENUA temperature change can predict whether a chemical reaction isendothermic or exothermic, considering the amount of heat utilized. Thisis in consideration with neglecting the effect of energy prior to and afterthe chemical reaction between the chemical species.A - If the first statement is TRUE and the second statement is FALSEB-If the first statement is FALSE and the second statement is TRUEC- If both statements are TRUEDIf both statements are FALSE↓|||()|18|♫

An increase in pressure favors a shift in the direction that will reduce the volume of the gas system, considering that the molecules are readily compressible. However, a change in solution pressure will have a negligible effect on the equilibrium. OA-If the first statement is TRUE and the second statement is FALSE OB-If the first statement is FALSE and the second statement is TRUE OC-If both statements are TRUE D-If both statements are FALSE

An increase in pressure favors a shift in the direction that will reduce the volume of the gas system, considering that the molecules are readily compressible. However, a change in solution pressure will have a negligible effect on the equilibrium. OA-If the first statement is TRUE and the second statement is FALSE OB-If the first statement is FALSE and the second statement is TRUE OC-If both statements are TRUE D-If both statements are FALSE

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...

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What is true about the forward and reverse reaction rates once chemical equilibrium is established? The reverse rate is always faster than the forward rate. Both the forward and reverse rates are equal Impossible to determine because it depends on the reaction. The forward rate is always faster than the reverse rate.
Give typed explanation
Although the equilibrium position changes as a result of a concentration or volume change, K does not. The statement is true. The statement is false. The statement can either be true and false. The statement is fallacious.
When a reaction's reaction quotient is smaller than its equilibrium constant, what does this indicate about the reaction's equilibrium? The reaction must proceed in the reverse direction to return to equilibrium. The reaction is at equilibrium and will not change. O The reaction must proceed in the forward direction to return to equilibrium. O Nothing. There is no relationship between the reaction quotient and equilibrium constant.
How would a drop in pressure effect a gaseous system at equilibrium? A. The reaction would shift to favor the side with the least moles of gas . B. The reaction would slow down , but the number of moles of gas would not change.
The molecule borneal can rearrange to a different form called isoborneal in a process called isomerization. A container initially contains only borneal gas at a pressure of 553 torr. At equilibrium, the pressure of borneall is 500.0 torr and the pressure of isoborneol is 53.0 torr. Is the isomerization reaction exergonic or endergonic? Calculate the value of the equilibrium constant for the reaction, borneal ⇌ isoborneol.
A system is considered to be at equilibrium. Which statement must be true? a) The reaction has stopped. b) The products and reactants are now equal in concentration. c) The reaction equilibrium state cannot be altered. d) There is no net change in the amount of reactant or product.
Suppose a flask is filled with of and of . The following reaction becomes possible: The equilibrium constant for this reaction is at the temperature of the flask. Calculate the equilibrium molarity of . Round your answer to two decimal places.
A student states that an equilibrium system is when the amount of reactants and products are equal. Is this true or false? Explain.
For which test tube should your value for the equilibrium constant be most reliable? Justify your selection based on your data and your laboratory experience in completing this procedure. Equilibrium Constant, K Test Tube 1 - 75.0 Test Tube 2 - 88.2 Test Tube 3 - 167 Test Tube 4 - 161 Test Tube 5 - -598 Average Kc = -21.4
2H₂S(g) = 2H₂(g) + S₂(g) A 6.82 g sample of H2S gas is heated in a 0.500 L rigid container. At equilibrium, 0.06605 mol H2 gas is present in the sealed container. Calculate the equilibrium concentration of S2(g) under these conditions. [S₂] = [?] mol/L S,, mol/L Enter