3 Ba (s) + 2 Al³ (aq)---->3 Ba*2(aq)2 Al (s)Al +3+3 eAl (s)E° -1.66 V @ 25°CBa 2(aq) + 2e--Ba (s)E° -2.90 V @ 25°CF-96, 485 C / mol e¨R 8.314J/mol * KWhat is the value of AG° for the above reaction?O-205 kJO-137 kJO-718 kJO+205 KjO+718 kJ

Step 1: Identify the half-cell reactionsStandard reduction potential from standard reduction…

Answered: 3 Ba (s) + 2 Al³ (aq) ----> 3 Ba*2(aq)…

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

The gas cyclopropane, C3H6(g), can be used in welding. When cyclopropane is burned in oxygen, the reaction is: 2 C3H6(g) + 9 O₂(g)6 CO₂(g) + 6 H₂O(g) (a) Using the following data, calculate AH° for this reaction. AH kJ mol-¹: C3H6(g) = 53.3; CO₂(g) = -393.5; H₂O(g) = -241.8 4 AH° = kj (b) Calculate the total heat capacity of 6 mol of CO₂(g) and 6 mol of H₂O(g), using CcO₂(g) = 37.1 J K-1 mol-¹ and CH₂O(g) = 33.6 J K-¹ mol-¹. C = JK-1 (c) When this reaction is carried out in an open flame, almost all the heat produced in part (a) goes to raise the temperature of the products. Assuming that the reactants are at 25°C, calculate the maximum flame temperature that is attainable in an open flame burning cyclopropane in oxygen. The actual flame temperature would be lower than this because heat is lost to the surroundings. Maximum temperature °℃
A hot, 3.00 g metal ball at 140.oC was placed in 8.0 mL of cold water at 12oC. The specific heat capacity of the metal is 3.3 J/g◦C. What was the final temperature of the water? [Hint: Look up the density of water.]
We want to convert 18 g of solid water at -22 °C to vapor at 116 °C. The energy need for this process is supplied by combustion of CH/C,H, gas mixture which is composed of 60% CH,(g) by mass. What is the volume of required amount of the mixture at 25 °C and under 745 mmHg pressure? For water c(solid) = 2.11 JgK", c(liquid) = 4.18 Jg" K", c(gas) = 2.00 J g K". AH"(fusion) = 6.00 kJ mol", AH (vapor.) = 40.7 kJ mol". %3D %3D %3D For CH, AH"(combustion) = -891 kJ mol %3D For C,He AH"(combustion) -1560 kJ mol O a. 1.38 L O b. 1.58 L Oc. 1.43 L O d. 1.47 L O e. 1.30 L
14. See image below. MM of Al:Os = 101.96 g/mol: 14. Calculate the amount of heat released in the complete combusti on of 8.17 grams of Al to form solid Alz03 at 25°C and 1 atm. AH for Al2O3 = 1676 kJ/mol 4Al) + 30(g) → 2Al:O: (5) 237 kJ O 254 kJ O 203 kJ O 127 kJ
us_engine.html?ClassID=1834324617# When a 4.25 g sample of solid NH4NO3 dissolves in 60.0 g of water in a coffee cup calorimeter, the temperature drops from 22.0°C to 16.9°C. What is the heat of reaction, qrxn? NH4NO3 ->>> NH+ + NO3 Csoln = 4.18 J/g °C arxn = [?] J Enter either a + or - sign AND the magnitude. Do not round until the end. q,soln (J) Enter
What volume (in mL) of benzene (C6H6, d= 0.88 g/mL, molar mass = 78.11 g/mol) is required to produce 2.38 x 10^3 kJ of heat according to reaction below? Report your answer to the nearest integer Reaction: 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) ΔH°rxn = -6278 kJ
An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g); ∆H = -1124 kJ. The density of sulfur dioxide at 25 °C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/mol °C. a) How much heat would be evolved in producing 1.00 L of SO2 at 25 °C and 1.00 atm? b) Suppose heat from this reaction is used to heat 1.00 L of SO2 from 25 °C to 500 °C for its use in the next step of the process. What percentage of the heat evolved is required for this?
Some commercial drain cleaners use a mixture of sodium hydroxide and aluminum powder. When the solid mixture is poured into the drain and dissolves, a reaction ensues that produces hydrogen gas: 2NAOH(aq) + 2AI(s) + 6H2O() → 2NAAI(OH)4(aq) + 3H2{g) Determine the temperature (in C) of hydrogen gas produced when 17.08 g of aluminum reacts with excess sodium hydroxide and water if the pressure is 107.37 kPa and the volume is 40.29 L. Provide your answer with TWO decimals.
The preparation of NO2(g) from N2(g) and O2(g) is an endothermic reaction: N2(g) + O2(g) -> NO2(g) (unbalanced) The enthalpy change of reaction for the balanced equation (with lowest whole-number coefficients) is ∆H = 67.7 kJ. If 250 mL of N2(g) at 100oC and 3.50 atm and 450 mL of O2(g) at 100oC and 3.50 atm are mixed, what amount of heat is necessary to synthesize NO2(g)?
For a particular isomer of CH, the combustion reaction produces 5099.5 kJ of heat per mole of C,H(g) consumed, under 18' 8 18 standard conditions. 25 02(g) 8 CO2(g)+9 H,0(g) AHn=5099.5 kJ/mol CH18 (g) + rxn 2 What is the standard enthalpy of formation of this isomer of CH(g)? 18 kJ/mol AHi
Give the correct answer for the attached question
Determine the amount of heat (in kJ) associated with the production of 3.20×104 g of ammonia according to the following equation. N2(g) + 3H2(g) 2NH3 ΔH°rxn = −92.6 kJ Assume that the reaction takes place under standard-state conditions at 25°C. Enter your answer in scientific notation. ______ x 10____ kJ

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

3 Ba (s) + 2 Al³ (aq) ----> 3 Ba*2(aq) 2 Al (s) Al +3 + 3 e Al (s) E° -1.66 V @ 25°C Ba 2(aq) + 2e-- Ba (s) E° -2.90 V @ 25°C F-96, 485 C / mol e¨ R 8.314J/mol * K What is the value of AG° for the above reaction? O-205 kJ O-137 kJ O-718 kJ O+205 Kj O+718 kJ

3 Ba (s) + 2 Al³ (aq) ----> 3 Ba2(aq) 2 Al (s) Al +3 + 3 e Al (s) E° -1.66 V @ 25°C Ba 2(aq) + 2e-- Ba (s) E° -2.90 V @ 25°C F-96, 485 C / mol e¨ R 8.314J/mol K What is the value of AG° for the above reaction? O-205 kJ O-137 kJ O-718 kJ O+205 Kj O+718 kJ