consider the following reaction CH3X + Y---> CH3Y + x at 25 degree celcius the following two experiments were run, yielding the following data: experiment 1 [Y]0=3M

[CH3X] time
7.08×10^-3 1
4.52×10^-3 1.5
2.23×10^-3 2.3
4.76×10^-4 4
8.44×10^-5 5.7
2.75×10^-5 7

Experiemtn 2 [Y]0=4.5M
[CH3X] time
4.5×10^-3 0
1.7×10^-3 1
4.19×10^-4 2.5
1.11×10^-4 4
2.81×10^-5 5.5
experiemtn also were run at 85 celcius. the value of the rate constant at 85 celcius was found to be 7.88×10^8(wiht the time in units of hours where [CH3X]= 1×10^-2M and [y]=3M

detemine the rate law and the value of k for this reaction at 25 celcius
determine the half life at 85 celcius
determine Ea for the reaction
fiven that C-E bond energy is known to be about 325 KJ/mol, suggest a mechanism that explain the results in parts a and c

im pretty sure i have to grpah it to find the straight line but my calculator stinks at graphing to find the order can some help me find the order and does it matter which exp i use to find the rate law and value of k? and can some help with d kinda have no clue=\

the time for the first are

1
1.5
2.3
4
5.7
7
and second is
0
1
2.5
4
5.5

i have the same ? ughhh did you get any of the problem yet.

To determine the rate law and the value of k for this reaction at 25 degrees Celsius, we can use the method of initial rates. In the method of initial rates, we compare the initial rates of reaction at different concentrations of reactants to determine their relationship.

Let's consider Experiment 1 first. We can start by calculating the initial rates of reaction at different concentrations of CH3X and Y.

For Experiment 1:
When [CH3X]0 = 7.08×10^-3 M, time = 1 s, the initial rate = ? (let's call it R1)
When [CH3X] = 4.52×10^-3 M, time = 1.5 s, the initial rate = ? (let's call it R2)
When [CH3X] = 2.23×10^-3 M, time = 2.3 s, the initial rate = ? (let's call it R3)

Now, we can compare the initial rates at different concentrations by taking the ratio of their rates:

R1/R2 = ([CH3X]0/[CH3X])
R2/R3 = ([CH3X]/[CH3X])

In both cases, Y is kept constant, so the ratio is only dependent on the concentration of CH3X.

Similarly, we can do the same for Experiment 2 at 25 degrees Celsius:

R4/R5 = ([CH3X]0/[CH3X])

By comparing these ratios, we can determine the order of the reaction with respect to CH3X. If the ratios are constant, then the reaction is zero-order with respect to CH3X. If the ratios depend on the concentration of CH3X, then the reaction is first-order or higher. We can use the data to determine the order experimentally.

Once we determine the order with respect to CH3X, we can do the same analysis for Y and determine its order as well. The overall rate law can be determined by multiplying the individual orders of CH3X and Y.

To find the value of k, we need to use one set of conditions where [CH3X]0 and [Y]0 are known, and the rate is measured. You can choose any set of conditions from the given experiments.

To determine the half-life at 85 degrees Celsius, we need the rate constant (k) at that temperature. You have mentioned that the rate constant at 85 degrees Celsius is 7.88×10^8, but you did not mention the units. Please provide the units so that we can proceed with the calculation.

To determine Ea (activation energy) for the reaction, we can use the Arrhenius equation:

k = A * e^(-Ea/RT)

where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant (8.314 J/mol·K), and T is the temperature in Kelvin.

To determine the suggested mechanism for the reaction, we need more information about the reaction conditions, reactants, and products. Please provide more details so that we can suggest a mechanism.

Regarding graphing the data, it is a useful approach to visualize the relationship between the reactant concentrations and the rate. You can plot a graph of concentration versus time for each reactant and check if it follows a linear relationship, indicating a certain order of the reaction.