a. Cis-`2`-butene `rarr` trans-`2`-butane, `DeltaH_(1)`
b. Cis-`2`-butane `rarr1`-butene, `DeltaH_(2)`
c. Trans-`2`-butene is more stable than `C` is-`2`-butene
d. Ethalpy of combustion of `1`-butene, `DeltaH =- 649.8 kcal//mol`
e. `9DeltaH_(1) +5DeltaH_(2) = 0`
f. Enthalpy of combustion of trans `-2`-butene, `DeltaH =- 647.1 kcal mol^(-1)`. Calculate `DeltaH_(1)`and `DeltaH_(2)`?

Explanation

To solve the problem, we need to calculate the values of ΔH₁ and ΔH₂ based on the given reactions and their enthalpy changes. Here's a step-by-step breakdown of the solution:

### Step 1: Understand the Reactions
We have the following reactions:
1. **Cis-2-butene → Trans-2-butene** with enthalpy change ΔH₁.
2. **Cis-2-butene → 1-butene** with enthalpy change ΔH₂.
3. **Trans-2-butene** is more stable than **Cis-2-butene**.
4. The enthalpy of combustion of **1-butene** is given as ΔH = -649.8 kcal/mol.
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