Final answer:
To determine the change in enthalpy (∆H) for the target reaction C(s) + H2O(g) → CO(g) + H2(g), we need to apply Hess's Law and sum the ∆H values of related reactions. However, without the exact ∆H value for the first reaction, the final ∆H cannot be calculated.
Step-by-step explanation:
To calculate the change in enthalpy (∆H) for the given reaction, we can use Hess's Law, which states that the total enthalpy change for a reaction is the same regardless of the number of steps the reaction is carried out in. If we know the enthalpy changes for related reactions, we can add or subtract these to find the enthalpy change for the overall reaction.
Lets examine the provided reactions:
- C(s) + H₂O(g) → CO(g) + H₂(g): This is the target reaction for which we are trying to find ∆H.
- 2 H₂(g) + O₂(g) → 2 H₂O(g), ∆H = -483.6 KJ: This is an additional reaction provided with a known ∆H value.
Now, let's arrange the equations to isolate the desired reaction:
- Reverse the second equation: 2 H₂O(g) → 2 H₂(g) + O₂(g), ∆H = +483.6 kJ (Reversing the reaction changes the sign of ∆H).
- Add the reversed second reaction to the first reaction:
C(s) + H₂O(g) + 2 H₂O(g) → CO(g) + H₂(g) + 2 H₂(g) + O₂(g)
Thus, the overall enthalpy change for the target reaction is the sum of the enthalpy changes of the first and reversed second reaction:
∆H₁ (unknown) + (+483.6 kJ) = ?
Without the exact value of ∆H for the first reaction, we cannot calculate the final ∆H of the target reaction. More information is needed to determine this value.