The water in a pressure cooker boils at a temperature greater than 100°C because it is under pressure. At this higher temperature, the chemical reactions associated with the cooking of food take place at a greater rate. (a) Some food cooks fully in 5 min in a pressure cooker at 112°C and in 10 minutes in an open pot at 100°C. Calculate the average activation energy for the reactions associated with the cooking of this food. (b) How long will the same food take to cook in an open pot of boiling water in Denver, where the average atmospheric pressure is 0.818 atm and the boiling point of water is 94.4°C?

The activation energy of a forward process is 65 kJ/mol, and that of the reverse process is 50 kJ/mol. What is ΔH of the process?

The activation energy (E) for the reaction 2N₂O(g) → 2N₂(g) + O₂(g) is 240.0 kJ mol kJ mol x10 What is the (E) for the reverse reaction? Round your answer to 3 significant digits. X AH° = -164 S kJ mol

The activation barrier for the hydrolysis of sucrose into glucose and fructose is 108 kJ/mol. If an enzyme increases the rate of the hydrolysis by a factor of (7.07x10^0)E6, how much is the activation energy of the catalyzed reaction? Assume the frequency (A) factors for the catalyzed and the uncatalyzed reactions are identical and the temperature is 25 deg. C. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer units

The hydrolysis of sucrose (C12H22O11)(C12H22O11) into glucose and fructose in acidic water has a rate constant of 1.8×10−4s−11.8×10−4s−1 at 25 ∘C∘C.Assuming the reaction is first order in sucrose, determine the mass of sucrose that is hydrolyzed when 2.65 LL of a 0.150 mol⋅L−1mol⋅L−1 sucrose solution is allowed to react for 195 minutes.

Thermal decomposition of substance A in the gas phase at a constant volume proceeds according to the equation A (g) → 3R (g). The reaction rate constant at 421°C is 3.10-4 s-1. How long from the start of the reaction does the concentration of substance R in the reaction mixture reach 50 times the concentration of substance A?

The rate constant for the reaction H2(g) + I2(g) → 2HI(g) is equal to 2.40 M–1 s–1 at 355 ºC and 9.80 M–1 s–1 at 385 ºC. Using these results, estimated the value of the rate constant at 415 ºC.

Chlorine dioxide (CO2) is a disinfectant used in municipal water treatment plants. It dissolves in basic solution producing ClO3 and CLO2: 2 ClO2(g) +2 OH(aq) → ClO3(aq) + ClO2 (aq) + H2O(l) The following kinetic data were obtained at 298 K for the reaction. Experiment [ClO2]0 (M) [OH]o (M) Initial Rate (M/s) 1 0.060 0.030 0.0248 2 0.020 0.030 0.00827 3 0.020 0.090 0.0247 Determine the rate law by indicating the values of "x" and "y" in the general rate law below. Rate = k[CO2]*[OH-] x= Select an answer✔ y = Select an answer b. Calculate the rate constant for this reaction at 298 K. Sig. Figs. are important. Rate constant, k = M-1 s-1

calculate the activation energy and the frequency factor of a certain reaction, using the tabulated data below

Calculate the rate constant, k, for a reaction at 73.0 °C that has an activation energy of 83.5 kJ/mol and a frequency factor of 2.53 x 10¹¹ s−¹. k= 8-1