For the reaction, 4 A(g) + 3 B(g) => 2 C(g), the following data were obtained at constant temperature.
Experiment Initial A, mol/L Initial B, mol/L Initial Rate, M/min
1 0.200 0.150 5.00
2 0.400 0.150 10.0
3 0.200 0.300 20.0
4 0.400 0.300 40.0
1. Determine the value of k for the reaction.
2. Which of the following is the correct rate law for the reaction?1. Rate = k[A]2[B]22. Rate = k[A][B]3. Rate = k[A]2[B]4. Rate = k[A][B]2

The k value for the reaction is k=5.56*10^3  M^-3/min and the rate law will be in order 3.

Explanation:

Finding the K value for the reaction

Write the rate equation,

Rate=K[A]*[A] [B]*[B]

Taking the rate values from the equation no 1 data

let K=5.00 M/min A=0.200 B=0.150

Rate=K[A]*[A] [B]*[B]

5.00 M/min = k(0.200)2(0.150)2 = 0.0009k

k = 5.00/0.0009

k=5556

k=5.56*10^3  M^-3/min

Then by solving the rate law we will get ,

The Rate law will be k[A]2[B]4.

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !