Answered: 2. Define and give an example:…

Science

Chemistry

2. Define and give an example: Spontaneous, exergonic 3. Define and give an example: Non-spontaneous, endergonic

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Does the entropy of the surroundings increase for spontaneous processes?
Spontaneous When entropy is positive and enthalpy is negative, a process is spontaneous. This means the reaction proceeds on its own under standard conditions, giving off energy as the reaction proceeds. Spontaneous at High Temperatures When entropy is positive and enthalpy is positive, a process is spontaneous at high temperatures because the products in the system are able to use thermal energy from the surroundings in order to react. Thermal energy increases the kinetic energy of the molecules. An example of this is ice melting. Ice will not melt if the temperature is not high enough. Spontaneous at Low Temperatures When entropy is negative and enthalpy is negative, a process is spontaneous at low temperatures. This type of reaction will release energy into the surroundings, and the ability to release this heat is important. If the temperature of the surrounding system is too high, the reactants have to overcome this energy in order to react and release their own heat energy. An…
According to the second law of thermodynamics for any spontaneous process, the entropy of the universe (increases, decreases, or remains constant)
Consider the following reaction at constant pressure. Use the information here to determine the value of AS surr at 298 K. Predict whether or not this reaction will be spontaneous at this temperature. N₂(g) +202(g) → 2NO₂(g) AHrxn = +88.4 kJ mol-1 ASsurr = +88.4J K-1 mol-1, reaction is spontaneous Assurr = -88.4J K-1 mol-1, reaction is spontaneous ASsurr = -88.4J K-1 mol-1, reaction is not spontaneous ASsurr = +297 J K-1 mol-1, reaction is spontaneous ⒸASsurr = -297J K-1 mol-1, reaction is not spontaneous
How does the entropy of the surroundings change duringan exothermic reaction? An endothermic reaction? Other thanthe examples in text, describe a spontaneous endothermic process
Use the standard free energy data to determine the free energy change for the following reactions, which is run under standard state conditions and 25 °C. Identify it as spontaneous or nonspontaneous at this condition. CASO2H;0(s) → CaSOds) + 2H¿O(g) AG (CaSO s)= -1322.0 kJ'mol 40 (HOg)--228.59 kl'mol AG(CasO-H;0,s) =.]797,45 kJ/mol 0 18.3kJ/mol, nonspontaneous 0-18.3kJ/mol, spontaneous 0 156kl/mol, nonspontaneous
Consider the reaction CaCO3(s)- →CaO(s) + CO₂(g) The standard free energy change for this reaction is 130.4 kJ. The free energy change when 1.87 moles of CaCO3(s) react at standard condition is 243.8 kJ. What is the maximum amount of useful work that the reaction of 1.87 moles of CaCO3(s) is capable of producing in surroundings under standard con ions? If no work can be done, enter none. kJ
5. Which of the following has a negative DS? A. Dissolve salt in water B. Heating chlorine vapors C. Heating a pure liquid D. Deposition of a gas to a solid 6. Which of the following has a negative DS? A. Melting ice B. Freezing liquid bromine C. Subliming a solid to a gas D. Evaporating water 7. What is defined as the phenomenon where the entropy of the universe increases in a spontaneous process and is constant in an equilibrium process? A. The law of spontaneity B. The 1st law of thermodynamics C. The 2nd law of thermodynamics D. The 3rd law of thermodynamics.
TRUE OR FALSE The spontaneous process proceeds on its own without any outside assistance.
What is a spontaneous process? Provide an example?
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