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Chemistry
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13 Dec 2019

Zn(s) + Hg2SO4(s) + 7H2O(l) --> ZnSO4.7H2O(s) + 2Hg(l)

A) what is the sign of the entropy change and what does this indicate about the reaction?

B) What is happening to cause the sign of the entropy change? And why is the magnitude of the entropy change so large?

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Hubert KochLv2
17 Dec 2019
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Related questions

(a) Does the entropy of the surroundings increase for spontaneous processes? (b) In a particular spontaneous process the entropy of the system decreases. What can you conclude about the sign and magnitude of ∆Ssurr? (c) During a certain reversible process, the surroundings undergo an entropy change, ∆Ssurr = –78 J/K. What is the entropy change of the system for this process?

(a) What sign for ∆S do you expect when the volume of 0.200 mol of an ideal gas at 27 °C is increased isothermally from an initial volume of 10.0 L? (b) If the final volume is 18.5 L, calculate the entropy change for the process. (c) Do you need to specify the temperature to calculate the entropy change? Explain.

A chemical reaction at equilibrium is heated, briefly, by holdingit over a flame. The equilibrium is seen to shift toward theproducts. What can be said about the enthalpy and entropy of thereaction?

Question 7 options:

We cannot determine the sign or the value of the entropychange


The entropy change must be negative, but we don't know thevalue


The entropy change must be positive, but we don't know thevalue


The enthalpy change cannot be determined


The enthalpy change could be negative (exothermic)


The enthalpy change could be positive (endothermic)


The sign of both the entropy and enthalpy change depends on thetemperature change

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