Consider the following reaction mechanism: Step 1: (CH3)3AuPH3 ↔ (CH3)3Au + PH3 (fast) Step 2: (CH3)3Au → C2H6 + (CH3)Au (slow) Step 3: (CH3)Au + PH3 → (CH3)AuPH3 (fast) What is the balanced equation for the overall reaction?

The balanced equation for overall reaction is:

(CH3)3AuPH3 > C2H6 + (CH3)AuPH3

Explanation:

The reaction mechanism is given as follows:

Step 1: (CH3)3AuPH3 ↔ (CH3)3Au + PH3 (fast)

Step 2: (CH3)3Au → C2H6 + (CH3)Au (slow)

Step 3: (CH3)Au + PH3 → (CH3)AuPH3 (fast)

To balance this equation, firstly, we conduct proper atom count for each steps of the reaction mechanism.

It is important to note that for a reaction that involves several steps, the rate law is normally derived from the slow step ( which is step2 from the above mechanism).

Therefore, the balanced chemical equation for the overall reaction is:

(CH3)3AuPH3 > C2H6 + (CH3)AuPH3

(CH3)3AuPH3 > C2H6 + (CH3)AuPH3

Explanation:

Firstly, to balance this equation, we conduct proper atom count for each steps of the reaction mechanism.

Step 1: (CH3)3AuPH3 ↔ (CH3)3Au + PH3 (fast)

Step 2: (CH3)3Au → C2H6 + (CH3)Au (slow)

Step 3: (CH3)Au + PH3 → (CH3)AuPH3 (fast)

It is important to note that for this reaction that involves several steps, the rate- determining step in the rate law is derived from the slow step which is seen in step2 from the above mechanism.

Thus, the balanced chemical equation for the overall reaction is:

(CH3)3AuPH3 > C2H6 + (CH3)AuPH3

i'm not sure

explanation:

i'll try whatever you got

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"