The reaction C,H, (g)2C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 x 10-8 s-1. What is the value of the rate constant at 730.0 K?

For the reaction A + B ---> C, the rate constant at 215°C is 5.0x10-3 M-1s-1and 1.2x10-1  M-1s-1at 452 °C. What is the activation energy for the reaction? [R=8.314 x 10-3kJ/mol.K]

The rate constant for the reaction is 0.200 M-! · s-! at 200 °C. A products If the initial concentration of A is 0.00780 M, what will be the concentration after 105 s? [A] = M * TOOLS x10

8. Dinitrogen tetraoxide (N2O4) decomposes spontaneously at room temperature in the gas phase: N2O4 (g) → 2 NO2(g) The rate law governing the disappearance of N2O4 with time is A[N,O4] = k N2O4]. At At 30°C, k = 5.1 x 106 s-1 and the activation energy for the reaction is 54.0 kJ/mol. Calculate the time (in seconds) required for the partial pressure of N2O4(g) to decrease from а. 0.10 atm to 0.010 atm at 30°C. b. Calculate the value of the rate constant at 300K. Repeat the calculation for the reaction in a) at the new temperature (300K). С. d. Write an observation about how the rate of reaction changed upon increasing the temperature.

Please don't provide hand writtin solution....

Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased

The reaction C₂H₂(g) → 2C₂H₂(g) - has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 x 10-8 s-1. What is the value of the rate constant at 820.0 K? k = 9.42 X10-26 Incorrect S-1

Consider the reaction: A + B --> products.  From the following data obtained at a certain temperature, determine the order of the reaction (rate law) and calculate the rate constant:   [A] (M)                       [B] (M)                       Rate (M/s)   1.50                             1.50                             3.15 X 10-1 1.50                             2.50                             2.98 X 10 –1 3.00                             1.50                             5.50 X 10-1