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Chapter 10: Q9DQ (page 396)

Is ΔSsurrfavourable or unfavourable for exothermic reactions and endothermic reactions? Explain.

Short Answer

Expert verified

ΔSsurr is favourable for an exothermic reaction while non-favourable for an endothermic reaction.

Step by step solution

01

ΔS for exothermic reaction

Primarily the entropy changes in the surroundings are determined by the flow of energy into or out of the system as heat.

In an exothermic process heat is supplied to the surrounding in form of thermal energy (kinetic energy). Due to the energy randomness of the atoms so entropy of surroundings increases.

ΔSsurr = +ve

Positive entropy means spontaneous process or favourable process. Thus, ΔSsurr is favourable for an exothermic reaction.

02

ΔS for endothermic reaction

During an endothermic process heat flows from surrounding to the system causing a decrease in randomness of the atoms in surroundings so entropy of surroundings decreases.

ΔSsurr = -ve

Negative entropy means non-spontaneous process or non-favourable condition. Thus, ΔSsurr is non- favourable for an endothermic reaction.

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Most popular questions from this chapter

Consider 1.00 mole of CO2(g) at 300 K and 5.00 atm. The gas expands until the final pressure is 1.00atm. For each of the following conditions describing the expansion, calculateq,w and ΔE.Cp for CO2 is 37.1JK-1mol-1, and assume that the gas behaves ideally.

  1. The expansion occurs isothermally and reversibly.
  2. The expansion occurs isothermally against a constant external pressure of 1.00atm
  3. The expansion occurs adiabatically and reversibly

Consider 1.00 mole of an ideal gas at 25°C.
a. Calculate q,w,∆E,∆S,∆Hand∆G for the expansion of this gas isothermally and irreversibly from 2.45×10-2 atm to 2.45×10-3 atm in one step.
b. Calculate for the same change of pressure as in part a but performed isothermally and reversibly.
c. Calculate localid="1649303003894" q,w,∆E,∆S,∆Hand∆Gfor the one-step so thermal, irreversible compression of 1.00 mole of an ideal gas at 25°C from 2.45×10-3atm to 2.45×10-3atm.
d. Construct the PV diagrams for the processes described in parts a, b, and c.
e. Calculate the entropy change in the surroundings for the processes described in parts a, b, and c.

Consider the following reaction at 35°C:
2NOCIg↔2NOg+Cl2gΔGo=20kJ
If 2.0 atm of NOClare reacted in a rigid container at 35°C, calculate the equilibrium partial pressure of NO .

Calculate ∆Ssurrfor the following reactions at 25°C and1 atm.

  1. C3H8(g)+5O2(g)→3CO2(g)+4H2O(I)∆H°=-2221kJ
  2. 2NO2(g)→2NO(g)+O2(g)∆H°=112kJ

Consider the relationship

In(K)=-ΔHoRT+ΔSoR

The equilibrium constant for some hypothetical process was determined as a function of temperature (in Kelvins) with the results plotted below

From the plot, determine the values of ΔHo and ΔSofor this process. What would be the major difference in the In(K)versus 1Tplot for an endothermic process as compared to an exothermic process?
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