QuestionPredict the sign of $\Delta S$ for each of these processes: Reaction $1.2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$ Reaction 2. $\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_{2} \mathrm{O}$ (s) Reaction 3. $\mathrm{CaCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$ Reaction 4. $\mathrm{CO}_{2}$ (s) $\rightarrow \mathrm{CO}_{2}$ (g) Reaction $5.2 \mathrm{C}_{8} \mathrm{H}_{18}(\mathrm{l})+25 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 16 \mathrm{CO}_{2}(\mathrm{~g})+18 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$
Reaction 1 [Choose]
Reaction 2 [Choose]
Reaction 3 [Choose]
Reaction 4 [Choose]
Reaction 5 [Choose]

Studdy Solution

STEP 1

1. Entropy change ( $\Delta S$ ) is related to the disorder or randomness of a system.
2. The phase change from gas to liquid or solid generally decreases entropy.
3. The phase change from solid or liquid to gas generally increases entropy.
4. The increase in the number of gas molecules typically increases entropy.
5. The decrease in the number of gas molecules typically decreases entropy.

STEP 2

1. Analyze each reaction to determine the phase changes and changes in the number of gas molecules.
2. Predict the sign of $\Delta S$ based on the analysis.

STEP 3

Reaction 1: $1.2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$
- Reactants: 1.2 moles of $\mathrm{H}_{2}(\mathrm{~g})$ and 1 mole of $\mathrm{O}_{2}(\mathrm{~g})$ = 2.2 moles of gas. - Products: 2 moles of $\mathrm{H}_{2} \mathrm{O}(\mathrm{l})$ = 0 moles of gas. - Gas to liquid transition decreases entropy.

STEP 4

Reaction 2: $\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{s})$
- Liquid to solid transition decreases entropy.

STEP 5

Reaction 3: $\mathrm{CaCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$
- Solid to gas transition increases entropy.

STEP 6

Reaction 4: $\mathrm{CO}_{2}(\mathrm{s}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})$
- Solid to gas transition increases entropy.

STEP 7

Reaction 5: $2 \mathrm{C}_{8} \mathrm{H}_{18}(\mathrm{l})+25 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 16 \mathrm{CO}_{2}(\mathrm{~g})+18 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$
- Reactants: 25 moles of $\mathrm{O}_{2}(\mathrm{~g})$ . - Products: 16 moles of $\mathrm{CO}_{2}(\mathrm{~g})$ and 0 moles of $\mathrm{H}_{2} \mathrm{O}(\mathrm{l})$ . - Decrease in the number of gas molecules decreases entropy.

STEP 8

Predict the sign of $\Delta S$ for each reaction:
Reaction 1: $\Delta S < 0$ (decrease in entropy) Reaction 2: $\Delta S < 0$ (decrease in entropy) Reaction 3: $\Delta S > 0$ (increase in entropy) Reaction 4: $\Delta S > 0$ (increase in entropy) Reaction 5: $\Delta S < 0$ (decrease in entropy)
Reaction 1: $\Delta S < 0$
Reaction 2: $\Delta S < 0$
Reaction 3: $\Delta S > 0$
Reaction 4: $\Delta S > 0$
Reaction 5: $\Delta S < 0$

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Studdy Solution

STEP 1

STEP 2

1. Analyze each reaction to determine the phase changes and changes in the number of gas molecules.
2. Predict the sign of $\Delta S$ based on the analysis.

STEP 3

STEP 4

Reaction 2: $\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{s})$
- Liquid to solid transition decreases entropy.

STEP 5

Reaction 3: $\mathrm{CaCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$
- Solid to gas transition increases entropy.

STEP 6

Reaction 4: $\mathrm{CO}_{2}(\mathrm{s}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})$
- Solid to gas transition increases entropy.

STEP 7

STEP 8

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Studdy Solution

STEP 1

STEP 2

1. Analyze each reaction to determine the phase changes and changes in the number of gas molecules.2. Predict the sign of ΔS\Delta SΔS based on the analysis.

STEP 3

STEP 4

Reaction 2: H2O(l)→H2O(s)\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{s})H2​O(l)→H2​O(s)- Liquid to solid transition decreases entropy.

STEP 5

Reaction 3: CaCO3( s)→CaO(s)+CO2( g)\mathrm{CaCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})CaCO3​( s)→CaO(s)+CO2​( g)- Solid to gas transition increases entropy.

STEP 6

Reaction 4: CO2(s)→CO2(g)\mathrm{CO}_{2}(\mathrm{s}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})CO2​(s)→CO2​(g)- Solid to gas transition increases entropy.

STEP 7

STEP 8

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1. Analyze each reaction to determine the phase changes and changes in the number of gas molecules.
2. Predict the sign of $\Delta S$ based on the analysis.

Reaction 2: $\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{s})$
- Liquid to solid transition decreases entropy.

Reaction 3: $\mathrm{CaCO}_{3}(\mathrm{~s}) \rightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})$
- Solid to gas transition increases entropy.

Reaction 4: $\mathrm{CO}_{2}(\mathrm{s}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})$
- Solid to gas transition increases entropy.