Predict the signs (-, +, or 0) of $\Delta$H and $\Delta$S, in that order, for the reaction: 6CO₂(g) + 6H₂O(g) $\rarr$C₆H₁₂O₆(g) + 6O₂(g). A) +, - B) 0, + C) +, + D) -, - E) None of the above

Question

Quizplus · Accepted Answer

To determine the signs of F1F1F1S1F1F1F10H and F1F1F1S1F1F1F10S, we need to look at the changes in entropy (S) and enthalpy (H) for the reaction.

From the balanced chemical equation, we see that there are more moles of gas on the right side of the equation than on the left. Therefore, the change in entropy is positive (S > 0).

For the enthalpy change, we need to use the bond dissociation energies of the reactants and products. The bonds broken in the reactants are C-O, H-S, and O=O. The bonds formed in the products are C-S, H-O, and S=O. Using these values, we can calculate the change in enthalpy to be negative (H < 0).

Using the signs for S and H, we can determine the signs of F1F1F1S1F1F1F10H and F1F1F1S1F1F1F10S as follows:

- If both S and H are negative, then F1F1F1S1F1F1F10H and F1F1F1S1F1F1F10S are both positive.
- If S is positive and H is negative, then F1F1F1S1F1F1F10H is negative and F1F1F1S1F1F1F10S is positive.
- If both S and H are positive, then F1F1F1S1F1F1F10H and F1F1F1S1F1F1F10S are both negative.
- If S is zero and H is negative, then F1F1F1S1F1F1F10H is negative and F1F1F1S1F1F1F10S is zero.
- If S is zero and H is positive, then F1F1F1S1F1F1F10H is positive and F1F1F1S1F1F1F10S is zero.

Therefore, the only choice that matches our predictions is A, + for F1F1F1S1F1F1F10S and - for F1F1F1S1F1F1F10H.

Predict the Signs (-, +, or 0) Of Δ\DeltaΔ H And Δ\DeltaΔ

Predict the Signs (-, +, or 0) Of $\Delta$ H And $\Delta$