Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- 1. Look at the attached reaction. What would you have to do to the reaction in order to increase the magnitude of K?arrow_forwardA2(g) + 3B2(g) -> 2AB3(g) where the ΔGorxn is -140 kJ and equilibrium constant at standard conditions is 3.5x1024. a) If we place 0.100 atm of AB3, 0.050 atm of B2, and 0.500 atm of A2 in a container at 25oC, which direction will the reaction go (if any) to reach equilibrium? b) What is the value of ΔGrxn assuming the temperature is maintained at 25oC?arrow_forwardGiven the thermodynamic properties below, determine the standard enthalpy change, ∆H˚, for the dissolution of calcium hydroxide. Give your answer to one decimal place in kJ/mol. 1 Ca(OH)2 (s) ⇌ Ca2+ (aq) + 2 OH– (aq)arrow_forward
- Calculate E∘cell�cell∘ for a redox reaction with n� = 2 that has an equilibrium constant of K� = 24 (at 25 ∘C∘C). Calculate ΔrG∘Δr�∘ for a redox reaction with n� = 2 that has an equilibrium constant of K� = 24 (at 25 ∘C∘C).arrow_forwardA reaction is studied at various temperatures, and a graph of ln K ( equilibrium constants on y axis) versus 1/T (Temperature on x axis) is prepared in Excel. The equation of the line is found to be y = - 9500 x + 21.5. What is the ΔSfor this reaction in J/mol/K? (assume R=8.314Jmol⋅K)arrow_forwardIf AG°rxn is 10.9 kJ/mol, determine AGrxn at 525 K, when TiCl4(g) = 0.250 atm. TiClą(liq) →TICI4(g)arrow_forward
- 8.B A certain reaction has an equilibrium constant of K = 8.3×10$ at 25°C with a temperature-independent standard enthalpy of reaction of 34.2 kJ/mol. (a) What is the equilibrium constant at 37°C? (b) Use Le Chatelier's principle to defend your answer.arrow_forwardDetermine the temperature of a reaction if K = 1.20 x 106 when AG° = +22.70 kJ/mol.arrow_forwardAmmonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N2(g) + 3H2(g) → 2NH3(g) Given that the standard free energy of formation of NH3 (g) is -104 kJ/mol at 298 K, calculate the equilibrium constant, K, at this temperature. To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3.arrow_forward
- Calculate delta G for the reaction, 2A (g) + B2(g) —- 2AB(g) given that at 120 C the equilibrium constant of the reaction is 3.12 x 10^5 -41.43 j/mol -41.43 kj/mol None of the above -35.76 kj/mol -414.30 j/molarrow_forwardCalculate the temperature at which the reaction below will be at equilibrium, then explain how this temperature can affect the spontaneity, meaning how using higher or lower than this temp can affect the value of delta G. Given. Br2(l) → Br2 (g), ΔH = 31.0 kj/mol ΔS = 92.9 j/molarrow_forward11. What is the ΔHº-value for the dissolution of NaOH (s) to yield 1.00... m NaOH (aq), given: Na (s) + 1/2 O2 (g) + 1/2 H2 (g) → NaOH (s) ΔHfº = -425.9 kJ/mol Na (s) + 1/2 O2 (g) + 1/2 H2 (g) → NaOH (aq, 1 m) ΔHfº = -469.2 kJ/mol Multiple Choice -895.1 kJ/mol -43.3 kJ/mol +1.102 kJ/mol +43.3 kJ/mol +895.1 kJ/molarrow_forward
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