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Part A Predict the sign of the entropy change, ΔS?, for each of the reaction displayed
Part A Predict the sign of the entropy change, ΔS?, for each of the reaction displayed.
Drag the appropriate items to their respective bins.
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Help Reset Ag+(aq)+Cl−(aq)→AgCl(s) 2KClO3(s)→2KCl(s)+3O2(g) 2N2O(g)→2N2(g)+O2(g) 2Mg(s)+O2(g)→2MgO(s) C7H16(g)+11O2(g)→7CO2(g)+8H2O(g) H2O(l)→H2O(g) Positive Negative |
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Part B
Calculate the standard entropy change for the reaction
2Mg(s)+O2(g)→2MgO(s)
using the data from the following table:
| Substance | ΔH?f (kJ/mol) | ΔG?f (kJ/mol) | S? [J/(K⋅mol)] |
| Mg(s) | 0.00 | 0.00 | 32.70 |
| O2(g) | 0.00 | 0.00 | 205.0 |
| MgO(s) | -602.0 | -569.6 | 27.00 |
Express your answer to four significant figures and include the appropriate units.
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| ΔS? = |
Expert Solution
Entropy is defined as:
Entropy = Entropy of products - Entropy of reactants
negative entropy: (Entropy of reactants greater than products)
Ag+(aq)+Cl−(aq)→AgCl(s)
2Mg(s)+O2(g)→2MgO(s)
Positive entropy: (Entropy of products is greater than reactants)
2KClO3(s)→2KCl(s)+3O2(g)
2N2O(g)→2N2(g)+O2(g)
C7H16(g)+11O2(g)→7CO2(g)+8H2O(g)
H2O(l)→H2O(g)
Part B
Entropy of reaction:
2Mg(s)+O2(g)→2MgO(s)
Entropy of products
MgO : 27, 2 MgO = 2 * 27 = 54 J / K mol
Entropy of reactants
2 Mg = 32.7 J / K mol
O2 = 205 J / K mol
Entropy of reaction : 54 - (32.7+205) = -183.7 J / K mol
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