Multiple Choice1. This overall reaction is best described as being:a. exothermicb. endothermicc. endergonicd. exergonice. spontaneous in the forward directiona. -35800 kJ/molb. 173.4 kJ/molc. 35800 kJ/mold. 101.7 kJ/mole. -274.2 kJ/mola. +0.46 Vb. +0.617 Vc. +1.39 Vd. -0.46 Ve.+1.21 VGa. 147 g Alb. 0.606 g Alc. 4.55 × 10-3 g AlReactants2. At 298 K, AH° for the following reaction is -137.5 kJ/mol, and AS° is +120.5 J/K.Calculate the value of AG° for this reaction at 298 K.C2H4 (g) + H2 (g) C2H6 (g)d. 16.4 g Ale. 49.1 g AlXReactants2Fe2+ (aq) + Sn4+ (aq)Products3. Use the Table to calculate the standard cell potential (Eºcell) for the voltaic cell basedon the reaction below.Sn2+(aq) + 2Fe3+, (aq)Reaction progressProductsHalf-reactionCr³+ (aq) + 3e-Fe2+ (aq) + 2e-Fe3+ (aq) + e- →Sn4+(aq) + 2e- →→Cr (s)Fe (s)Fe2+ (s)Sn²+ (aq)4. How many grams of aluminum metal are produced in the electrolysis of molten AIC13for 3.25 br with an electrical current of 15.0 A.Al³+ + 3e- Al(s)E° (V)-0,74-0.440+0.771+0.154

Answered: Image /qna-images/answer/f6074dda-1833-416e-886d-172522e50467.jpg

Multiple Choice 1. This overall reaction is best described as being: a. exothermic b. endothermic c. endergonic d. exergonic e. spontaneous in the forward direction a. -35800 kJ/mol b. 173.4 kJ/mol c. 35800 kJ/mol d. -101.7 kJ/mol e. -274.2 kJ/mol G Reactants a. +0.46 V b. +0.617 V c. +1.39 V d. -0.46 V e. +1.21 V Reactants 2. At 298 K, AH° for the following reaction is -137.5 kJ/mol, and AS° is +120.5 J/K. Calculate the value of AG for this reaction at 298 K. C2H4 (g) + H2 (g) C2H6 (g) Products Reaction progress Products 3. Use the Table to calculate the standard cell potential (Eºcell) for the voltaic cell based on the reaction below. Sn²+ (aq) + 2Fe3+ (aq) → 2Fe²+ (aq) + Sn4+ (aq) Half-reaction Cr³+ (aq) + 3e → Cr (s) Fe2+ (aq) + 2e →→ → Fe (s) Fe2+ (s) Fe³+ (aq) + e- → Sn4+ (aq) + 2e- Sn²+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154

Multiple Choice 1. This overall reaction is best described as being: a. exothermic b. endothermic c. endergonic d. exergonic e. spontaneous in the forward direction a. -35800 kJ/mol b. 173.4 kJ/mol c. 35800 kJ/mol d. -101.7 kJ/mol e. -274.2 kJ/mol G Reactants a. +0.46 V b. +0.617 V c. +1.39 V d. -0.46 V e. +1.21 V Reactants 2. At 298 K, AH° for the following reaction is -137.5 kJ/mol, and AS° is +120.5 J/K. Calculate the value of AG for this reaction at 298 K. C2H4 (g) + H2 (g) C2H6 (g) Products Reaction progress Products 3. Use the Table to calculate the standard cell potential (Eºcell) for the voltaic cell based on the reaction below. Sn²+ (aq) + 2Fe3+ (aq) → 2Fe²+ (aq) + Sn4+ (aq) Half-reaction Cr³+ (aq) + 3e → Cr (s) Fe2+ (aq) + 2e →→ → Fe (s) Fe2+ (s) Fe³+ (aq) + e- → Sn4+ (aq) + 2e- Sn²+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154

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

Please do this...
Select all the inequalities below that correspond to exothermic reactions or processes. A. ΔH > 0 B. q < 0 C. ΔH < 0 D. q > 0 (you can select more than one)
For a certain process at 455 K, A G=-12.1 kJ and A H=-9.2 kJ. Therefore, A S for the Oa. 6.37 J/K mol process is Ob.0 J/K mol Oc. 3.98 J/K mol d. 8.2 J/K mol O e.-8.2 J/K mol
Indicate whether each process is spontaneous or nonspontaneous. a. water vapor condensing at 50 °C b. salt crystallizing from an unsaturated solution. c. a cold drink warming up in the hot sun d. carbon dioxide bubbling out of a warm soda e. salt and sand particles separating themselves in a mixture f. all the oxygen in a room condensing at one spot
I. MULTIPLE CHOICE Read and answer each question carefully. Write your answer in the space provided. 3. Which of the following statements are true for the reaction: I(e)> 21e) AH is positive AH is negative AS is positive AS is negative The reaction is spontaneous in any temperature I. П. III. IV. V. а. I and II b. I only с. IV only d. V only e. II and III
a. H₂O b. SH- c. S²- BH3 e. NH3 14. At what temperatures will a reaction be spontaneous if A,H=+117 kJ and A,S = -35 J/K? The reaction will be spontaneous at any temperature. b. The reaction will never be spontaneous. c. Temperatures between 12.7 K and 135 K d. All temperatures above 94.1 K e. All temperatures below 94.1 K
D. H20 (s) –> H20 (I) AHo = 6.01kJ/mol| 1. This reaction depicts the 2. Is this reaction endothermic or exothermic? 3. Is this reaction reversible or irreversible? (process) of (product).
If the process is exothermic and not spontaneous, then what must be TRUE? O a. AS0 O c. AH=0 O d. AS> 0
In a reaction similar to Reaction 1, 3.2 g of sodium hydroxide (NaOH) is added to 100.0 g of water. A rise in temperature of 2.9 °C was noted. Assume the solution formed is water and c= 4.184 J/ (g °C). a. Calculate the heat, q, evolved for this reaction. b. How many moles of NaOH were reacted? c. Using the answers to a and b, what is the H for this reaction in kJ/mol?
9- " Systems that are in thermal equilibrium exist at the same temperature". This statement is according to :- Oa- First law of thermodynamics. O c- Zeroth law of thermodynamics Od- Third law of thermodynamics. Ob- Second law of thermodynamics.
4. Select all that is considered spontaneous a. Cleaning your room b. A piece of bread molding after being left out in the sun c. A bomb exploding d. Pushing a ball up a ramp e. Ice melting f. Frying an egg g. Putting together a puzzle