For the reaction, A(g) + 2B(g) → 2C(g) + 2D (g) the following data was collected at constant temperature. Determine the correct rate law for this reaction.

Trial
Initial [A]
Initial [B]
Initial Rate

(mol/L)
(mol/L)
(mol/(L·min))
1
0.125
0.200
7.25
2
0.375
0.200
21.75
3
0.250
0.400
14.50
4
0.375
0.400
21.75
E) Rate = k[A]3
C) Rate = k[A] [B]2
A) Rate = k[A] [B]
D) Rate = k[A]
B) Rate = k[A]2 [B]

personal, she chose to do it.

answer : third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol

explanation :

let us write down the given equations

equation 1 :

equation 2 :

equation 3 :

let us use hess's law to find out which 2 equations can be added to get the third equation.

let us reverse equation 2 and multiply it by 2. the new equation that we get is,

equation 4 :

let us add equation 1 & 4

the above equation is similar to equation 3 but has different value for dhrxn.

therefore third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol

the answer is 0.42 is that is an option. this question provides no info