ellumHMAC=e84666a38b6ed866c9d641cbecc78b80#10001 11 of 44 Review | Constants | Periodic Table Part D A student sets up two reactions. Reaction 1 uses 0.250 mol/L of reactant, and Reaction 2 uses 0.410 mol/L of reactant. How many times faster is Reaction 2 compared to Reaction 1? Express your answer as a multiple of the rate for Reaction 1 to three significant figures. Note that Reaction 1 is already written for you, so just enter the number. ▾ View Available Hint(s) ▼ Hint 1. Setting up the ratio Since 0.410/0.250 = 1.64, the second reaction contains 1.64 times the amount of reactant compared to Reaction 1. The reaction rate is proportional to the square of the amount of reactant, so the rate will increase by a factor of the square of 1.64. VO 5 ? rate of Reaction 2 X rate of Reaction 1 Mal | ΑΣΦ 8 an 3:28 PM

ellumHMAC=e84666a38b6ed866c9d641cbecc78b80#10001 11 of 44 Review | Constants | Periodic Table Part D A student sets up two reactions. Reaction 1 uses 0.250 mol/L of reactant, and Reaction 2 uses 0.410 mol/L of reactant. How many times faster is Reaction 2 compared to Reaction 1? Express your answer as a multiple of the rate for Reaction 1 to three significant figures. Note that Reaction 1 is already written for you, so just enter the number. ▾ View Available Hint(s) ▼ Hint 1. Setting up the ratio Since 0.410/0.250 = 1.64, the second reaction contains 1.64 times the amount of reactant compared to Reaction 1. The reaction rate is proportional to the square of the amount of reactant, so the rate will increase by a factor of the square of 1.64. VO 5 ? rate of Reaction 2 X rate of Reaction 1 Mal | ΑΣΦ 8 an 3:28 PM

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.35QE

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Similar questions

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.
5.12. True or false: If all the partial pressures of reactants and products drop by half, the value of Q drops by half. Give an example of a chemical reaction to support your answer.
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. 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?
The boxes shown below represent a set of initial conditions for the reaction: Draw a quantitative molecular picture that shows what this system looks like after the reactants are mixed in one of the boxes and the system reaches equilibrium. Support your answer with calculations.
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?
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.
Hydrogen sulfide is a pollutant found in natural gas. Following its removal, it is convened to sulfur by the reaction 2H2S(g)+SO2(g)38S8(s,rhombic)+2H2O(l). What is the equilibrium constant for this reaction? Is the reaction endothermic or exothermic?
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What happens to the reactants in an ineffective molecular collision?
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