When 100. mL of 1.0 M HCl is added toa 2.0 g piece of CACO3, CO2 is producedat a certain rate. Which of the changesbelow will NOT increase the rate of thisreaction?a. Adding 100, mL of 2.0 M HCl inplace of 100. mL of 1.0 M HCI.b. Heating the 100. mL of 1.0 MHCl before adding it to theСаСОз.c. Adding 100. mL of 1.0 M HCl to2.0 g of powdered CaCO3.d. Adding 150. mL of 1.0 M HCl inplace of 100. mL of 1.0 M HCI.

In a 2 g piece of CaCO3 , 100 mL of 1M HCl is added, which produces CO2. We need to find out the…

to en 100. mL of 1.0 M HCI is added to a 2.0 g piece of CaCO3, CO2 is produced at a certain rate. Which of the changes below will NOT increase the rate of this When М НСПIS reaction? a. Adding 100. mL of 2.0 M HCl in place of 100. mL of 1.0 M HCl. b. Heating the 100. mL of 1.0 M HCl before adding it to the СаСОз. c. Adding 100. mL of 1.0 M HCl to 2.0 g of powdered CaCO3. d. Adding 150. mL of 1.0 M HCl in place of 100. mL of 1.0 M HCI.

to en 100. mL of 1.0 M HCI is added to a 2.0 g piece of CaCO3, CO2 is produced at a certain rate. Which of the changes below will NOT increase the rate of this When М НСПIS reaction? a. Adding 100. mL of 2.0 M HCl in place of 100. mL of 1.0 M HCl. b. Heating the 100. mL of 1.0 M HCl before adding it to the СаСОз. c. Adding 100. mL of 1.0 M HCl to 2.0 g of powdered CaCO3. d. Adding 150. mL of 1.0 M HCl in place of 100. mL of 1.0 M HCI.

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 129MP: A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A...

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A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.
Why are there no changes specified for Ni in Exercise 13.61, part (f)? What property of Ni does change?
In the text, the equation G=G+RTIn(Q) was derived for gaseous reactions where the quantities in Q were expressed in units of pressure. We also can use units of mol/L for the quantities in Q, specifical.ly for aqueous reactions. With this in mind, consider the reaction HF(aq)H+(aq)+F-(aq) for which Ka = 7.2 104 at 25C. Calculate G for the reaction under the following conditions at 25C. a. [HF] = [H+] = [F] = 1.0 M b. [HF] = 0.98 M, [H+] = [F] = 2.7 102M c. [HF] = [H+] = [F] = 1.0 105 M d. [HF] = [F] = 0.27 M, [H+] = 7.2 104M e. [HF] = 0.52 M, [F] = 0.67 M, [H+] = 1.0 103M Based on the calculated G values, in what direction will the reaction shift to reach equilibrium for each of the five sets of conditions?
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.
Calculate G for the dissolution of both sodium chloride and silver chloride using data from Appendix E. Explain how the values you obtain relate to the solubility rules for these substances.
Substances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?
. Before two molecules can react, chemists envision that the molecules must first collide with one another. Is collision among molecules the only consideration for the molecules to react with one another?
7-17 If a certain reaction takes 16 h to go to completion at 10°C, what temperature should we run it if we want it to go to completion in 1 h?
When molecules collide, a certain minimum energy called the _________ is needed for the reaction to occur.
Determine rxnH 25 C for the following reaction: NO g O2 g NO2 g This reaction is a major participant in the formation of smog.
The only stress (change) that also changes the value of K is a change in temperature. For an exothermic reaction, how does the equilibrium position change as temperature increases, and what happens to the value of K? Answer the same questions for an endothermic reaction. If the value of K increases with a decrease in temperature, is the reaction exothermic or endothermic? Explain.
12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial concentrations are [O3]=1.0106M,[NO]=1.0105M,[NO2]=2.5104M, and [O2]=8.2103M , is the system at equilibrium? If not, in which direction does the reaction proceed? (b) If the temperature is increased, as on a very warm day, will the concentrations of the products increase or decrease? (HINT: You may have to calculate the enthalpy change for the reaction to find out if it is exothermic or endothermic.)