aA certain catalyzed reaction is known to have an activation energy E₁ = 17.0 kJ/mol. Furthermore, the rate of this reaction is measured at 299. K and found tobe 1.1 × 105 M/s. Use this information to answer the questions in the table below.Suppose the concentrations of all reactants iskept the same, but the temperature is loweredby 10% from 299. K to 269. K.How will the rate of the reaction change?Suppose the concentrations of all reactants iskept the same, but the catalyst is removed,which has the effect of raising the activationenergy by 5%, from 17.0 kJ/mol to17.9 kJ/mol.How will the rate of the reaction change?The rate willThe rate will✓ choose onestay the samerise about 10%rise more than 10%rise less than 10%fall about 10%fall more than 10%fall less than 10%☑

1. The rate of a chemical reaction is strongly dependent on temperature, as described by the…

Answered: a A certain catalyzed reaction is known…

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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4. A certain chemical reaction has a rate constant of 1.50 L/mol·min at 45.0°C with an activation energy of 108.0 kJ/mol. Calculate the value of the rate constant for the reaction at 60.0°C.
A certain reaction is known to have an activation energy E= 9.0 kJ/mol. Furthermore, the rate of this reaction is measured at 350. K and found to be 4.5 x 10° M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is raised by 5% from 350. K to 368. K. How will the rate of the reaction change? The rate will choose one choose one stay the same rise about 5% rise more than 5% rise less than 5% fall about 5% fall more than 5% fall less than 5%
The rate of a certain reaction is given by the following rate law: rate =k[N,]H, ° Use this information to answer the questions below. olo What is the reaction order in N,? x10 Ar What is the reaction order in H,? What is overall reaction order? At a certain concentration of N, and H2, the initial rate of reaction is 0.090 M / s. What would the initial rate of the reaction be if the concentration of N, were doubled? Round M S your answer to 2 significant digits. The rate of the reaction is measured to be 95.0 M / s when [N2] = 0.99 M and [H2] = 1.1 M. Calculate the value of the -2 -1 k = •S rate constant. Round your answer to 2 significant digits.
A certain catalyzed reaction is known to have an activation energy E 9.0 kJmol. Furthermore, the rate of this reaction is measured at 354. K and found to be 4.7 x 10 M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature 5% from 354. K to 372. K. raised by choose one The rate will How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 5%, from 9.0 kJ/mol to 9.45 kJmol choose one The rate will choose one How will the rate of the reaction change? stay the same rise about 5% rise more than 5% rise less than 5% fall about 5% fall more than 5% fall less than 5%
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 398.0 °C 8.9 x 10' 262.0 °C 8.0 x 106 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E = x10 mol X S C.
A certain reaction has an activation energy of 43.99 kJ/mol. At what Kelvin temperature will the reaction proceed 4.00 times faster than it did at 353 K?
A student collected conducted 6 kinetics experiments for one reaction by holding the concentrations of ALL the reactants and catalyst constant and varying the temperature. After determining the rate constant for this reaction at the 6 different temperatures, an Arrhenius Plot was made. The graph resulted in a straight line. The equation for the straight line was: y= -3,378.84 x + 14.326 What is the Activation Energy (in Joules/mol) for this reaction at 30 oC? Do not include the units in your answer.
A particular reaction has an activation energy, Ea, of 189 kJ/mol. If the rate constant for the reaction is 0.00205 s−1 at 457 °C, at what temperature (°C) would the rate constant be 0.200 s−1?
The rate of a reaction becomes four times when the temperature changes from 293 K to 313 K. Calculate the energy of activation (Ea) of the reaction assuming that it does not change with temperature.[R = 8.314 J K-1 mol-1, log 4 = 0.6021]
A certain catalyzed reaction is known to have an activation energy E= 11.0 kJ/mol. Furthermore, the rate of this reaction is measured at 296. K and found to be 1.1 × 10 M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is raised by 10% from 296. K to 326. K. How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 5%, from 11.0 kJ/mol to 11.6 kJ/mol. How will the rate of the reaction change? The rate will The rate will choose one choose one choose one stay the same rise about 5% rise more than 5% rise less than 5% fall about 5% fall more than 5% fall less than 5% V
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 59.0 °C 6.5 x 101 14 163.0 °C |4.2 × 10 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. a Round your answer to 2 significant digits. kJ E x10 mol
The reaction C4H8(g)⟶2C2H4(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, ?, is 6.1×10−8 s−1. What is the value of the rate constant at 855.0 K?

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