The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E = 19.0 kJ/mol. If the rate constant of this reaction is 2.5 × 10° M's -1 at 343.0 °C, what will the rate constant be at 310.0 °C? Round your answer to 2 significant digits. -1 k = | M

TIA

Calculate the average rate of a reaction, given the following data: Reaction Data Time (s) Concentration (mol/L) 60 5.00 × 10-² 85 3.25 x 10-²

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 142.0 °C 6.1 x 1011 226.0 °C 3.7 x 10¹2 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. mol ×

A certain catalyzed reaction is known to have an activation energy E =39.0 kJ/mol. Furthermore, the rate of this reaction is measured at 278. K and found to be 4.7 × 10² 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 lowered by 10% from 278. K to 250. 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 39.0 kJ/mol to 41.0 kJ/mol. How will the rate of the reaction change? The rate will 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 constant k for a certain reaction is measured at two different temperatures: temperature 274.0 °C 348.0 °C E = a Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a k 4.2 × 10 ¹0 11 1.8 × 10¹ Round your answer to 2 significant digits. kJ mol x10 X Ś

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 70.0 °C 5.6 x 107 -63.0 °C 3.1 × 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 = mol O2022 McGraw Hill LLC. All Rights Reserved. Te 43,203 FEB 18 CH.9 PP ASSESS MacBook Air

Only typed solution.

One mechanism for the destruction of ozone in the upper atmosphere is Os (9) + NO(g) → NO₂(g) + O2(g) Slow NO₂(g) + 0(g) → NO(g) + O₂(g) Fast Overall reaction O3(g) + O(g) → 20₂ (g) a. Which species is a catalyst? ONO 003 002 O NO2 b. Which species is an intermediate? ONO 003 002 O NO₂ c. E₂ for the uncatalyzed reaction 03 (g) + 0(g) → 20₂ (g) is 14.0 kj. E for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 85°C? Assume the frequency factor A is the same for each reaction. Ratio = [References) Submit Answer Try Another Version frem atempt remaning (Pr Previous

General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning The reaction C,H, (g) → 2 C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-1. What is the value of the rate constant at 750.0 K? k = 1.34 x103 Incorrect