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.

g) K2CO3 + HNO3 → Type of reaction h) BİCI3 + КОН Type of reaction NaC2H3O2 + COSO4 -> I) Type of reaction

1. The shape of boron trihydride, BH3, is 2. In an exothermic reaction, the potential energy of the products is than the potential energy of the reactants. 3. A system at equilibrium always has forward and reverse reaction rates which are 4. A solution at 25°C with a pOH of 3.45 has a pH of 5. When nitric acid is titrated to an end point by lithium hydroxide, two products are and O 6. The standard reduction potential table lists the Evalues of half-cell reactions measured in combination with the standard half-cell.

Given each equilibrium constant, state whether the reactants are favored, the products are favored, or both the reactants and products are present at equilibrium. a. 5.0 × 10 −4 b. 4.4 × 10 5 c. 350 d. 0.35

1. Monitoring blood glucose levels is an important aspect of managing diabetes. The preprandial glucose level is the glucose level measured before a meal, and it should be 70 - 130 mg/dL. When testing blood glucose levels in a laboratory, two reactions are implemented to determine the concentration of glucose in the blood. First, glucose is broken down in the presence of water and oxygen by the enzyme glucose oxidase to form hydrogen peroxide and gluconic acid. When 4-aminoantipyrine and p-hydroxy benzene sulfonic acid (p-HBS) is added in the presence of peroxidase, the hydrogen peroxide is converted to water and a red quinone imine dye. The concentration of the dye can be measured spectrophotometrically and related back to the initial concentration of glucose. Glucose Oxidase C6H1206 + H20 + 02 glucose H202 + C6H1207 gluconic acid Peroxidase H202 + C11H13N30 + C6 H,04S 4-aminoantipyrine p-HBS H20 + Quinone Imine Dye After both reactions have come to completion, the concentration of…

Consider the exothermic reaction: A (g) + B (s) → 2X (g) @ 25 °C a. Propose a change in VOLUME so that the equilibrium position shifts towards the REACTANTS. b. Propose a change in TEMPERATURE so that the equilibrium position shifts towards the PRODUCTS. c. Propose a change in [A] so that the equilibrium position shifts towards the PRODUCTS.

Consider the following: N2(g)+ 3H2(g) = 2NH3(g) Ke= 6.3 × 10° What is the new K, for this reaction but I rewrite it to show the production of 1 mole of H2 and 0.333 moles of N2 from 0.666 moles of NH3? A. 2.10 x 108 B. 1.17 x 103 C. 1.36 × 103 D. 3.99 x 10-27

I. 2NOCl (g)< < >  2NO(g) + Cl2(g)                   K= 1.6X 10-5 II. 2NO (g)  < > N2(g) + O2(g)                       K= 1.0 X 1031 Which of the following will you choose to generate the most amount of NO? (Think which of the reactions will favor the formation of NO.)a.Forward reaction of IIb.Forward reaction of Ic.Reverse reaction of Id.Reverse reaction of II

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If the equilibrium constant, K, is greater than 1 which of the following is true? Select one: a. There are more products than reactants. b. There are more reactants than products. O c. We have all reactants and zero products. O d. The number of reactants equals the number of products.