Which stateueut is false? (a) Ifa reaction is thermodynamically spontaneous it may occur rapidly. (b) If a reaction is thermodynamically spontanoous it may occur slowly. (c) Activation energy is a kinetic quantity rather than a thermodynamic quantity. (d) If a renction is thermodynamically nonspontanoous, it will not occur spontaneously. (e) Ifa reaction is thermodynamically spontaneous, it must have a low activation energy

Which stateueut is false? (a) Ifa reaction is thermodynamically spontaneous it may occur rapidly. (b) If a reaction is thermodynamically spontanoous it may occur slowly. (c) Activation energy is a kinetic quantity rather than a thermodynamic quantity. (d) If a renction is thermodynamically nonspontanoous, it will not occur spontaneously. (e) Ifa reaction is thermodynamically spontaneous, it must have a low activation energy

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...

See similar textbooks

Similar questions

(d) For the reaction: H3C. H3C. C-OH Cc=CH2 H3C H20 H,C H3C Reaction 2 Reaction 2 does not go to completion and the position of the reaction can be defined in terms of the equilibrium constant, K. (i) For the above reaction at 298K under specific conditions the following thermodynamic information were obtained, reaction Gibbs free energy (AreactG = -5.4 kJ mol-1), standard reaction enthalpy (AreactH® = -52.7 kJ mol-1) and standard reaction entropy (AreactS® = -0.16 kJ mol-1). From the above detail, calculate the equilibrium constant. (ii) Sketch a diagram of the Gibbs free energy versus reaction progress and on diagram label the reaction Gibbs free energy (A,react G) and standard reaction Gibbs free energy (Areact G®).
Be sure to answer all parts. Use the table to caleulate AG"_ for the following reactions at 25°C. Species AG (kJ/mol) Mg(s) 0:(8) MgO(s) -569.6 SO,(8) -300.57 so,(3) |-370.53 C,H2(3) 209.2 CO2(3) -394.65 H,O() -237.35 H,O(g) -228.77 (a) 2 Mg(s) + O2(g) →2 MgO(s) kJ (b) 2 SO¿(g) + O2(g) → 2 SO3(g) kJ (c) 2 C,H¿(g) + 5 O,®) → 4 CO,(g) + 2 H,0) kJ
(a) Using Gibb's free energy equation, predict whether at 28.0 °C, the following reaction is spontaneous or not: 4 NH3 (g) + 5 O2 (g) 4 NO (g) + 6 H2O (g) (Given: AU = + 9.08 kJ.mol¬' and AS = + 35.7 JK-' mol-') Hint: Use AU and above equation to calculate AH first. (b) Calculate the Change in Gibb’s Free energy for the following reaction and predict whether the reaction is spontaneous under standard conditions or not? 4 KCIO3 (9) — ЗКСІО4 (9) + КCІ () Given: Molecules дн? (кJ/mol) S°(J/mol.K) KCIO3 (s) -397.7 143.1 KCIO4 (s) -432.8 151.0 KCI (s) -436.7 82.6
How would I solve this question?
When dry ice (solid CO 2) sublimates, its entropy(A) increases(B) decreases(C) does not change(D) could either increase or decrease, depending on other factors
If K is postive than one (reactant favored), then AGO is greater;spontaneous equal; non spontaneous less; nonspontaneous less; spontaneous
(a) Does the entropy of the surroundings increase for spontaneousprocesses? (b) In a particular spontaneous processthe entropy of the system decreases. What can you concludeabout the sign and magnitude of ΔSsurr? (c) Duringa certain reversible process, the surroundings undergo anentropy change, ΔSsurr = -78 J/K. What is the entropychange of the system for this process?
State if each of the following processes is spontaneous, not spontaneous, or if additional information is needed to give an answer. Make sure that you detail whatadditional information you need in order to decide.(A) A process at constant temperature and pressure for which ∆S of the system ispositive.(B) A process for which ∆S is negative and ∆Ssurr is positive.(C) A process for which ∆S is negative and ∆Ssurr is zero.
(a) Define what is spontaneous reaction. (b) How it is related to chemistry
(a) What is a spontaneous process? Explain, with a simple quantitative example, why the flow of heat from a hot to a cold body is spontaneous but the reverse is not. (b) “Entropy is the tax we pay for borrowing Nature’s power”. Discuss. (c) Arthur Edington described entropy as “the arrow of time”. Explain what Edington meant.
a) b)
For the reaction CO (g) + H,O (g) → CO-(g) + H2 (g), calculate the following reaction's thermodynamic variables: