For the reaction 2N2O3(g) → 4NO2(g) + O2(g), the following data were collected: 1 (minutes) [N2O5] (mol/L)
0 1.24 x 10-2
10. 0.92 x 10-2
20. 0.68 x 10-2
30.
0.50 x 10-2
40. 0.37 x 10-2
9
50.
0.28 x 10-2
0.15 x 10-2
70.
The initial rate of production of NO2 for this reaction is approximately:
O a. 7.4 x 10-4 mol/L min
O b. 3.2 x 10-4 mol/L min
O c. 1.24 x 10-2 mol/L min
O d. 1.6 x 10-4 mol/L'min
e.
none of these

65uuyhjghj8ykitdyidii

with this one i know the answer in craters one reason i looked it up and i learned about it there is my evidence

it is b that is the answer.

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