Using thermodynamic data to calculate K Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. TiCl 4 (g) + 2H2O(g) →>> TiO2 (s) + 4 HCl (g) Round your answer to 2 significant digits. K = [] ☐ x10 ☑ ? 00. 18 Ar Al-

Using thermodynamic data to calculate K Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. TiCl 4 (g) + 2H2O(g) →>> TiO2 (s) + 4 HCl (g) Round your answer to 2 significant digits. K = [] ☐ x10 ☑ ? 00. 18 Ar Al-

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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Calculate AGO at 605 K for H₂O(g) + 1/2 02(g) → H₂O₂(g) using the following data: AGO = H₂(g) +O₂(g) → H₂O₂(g) K = 8.9 × 10³6 at 605 K 2H₂(g) + O₂(g) → 2H₂O(g) K = 2.0 x 106 at 605 K kJ/mol
Consider the following chemical equilibrium: C(s) + 2 H₂ (g) ⇒ CH₂(g) Now write an equation below that shows how to calculate K from K for this reaction at an absolute temperature T. You can assume I is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K -0 X 00
Using any data you can find in the ALEKS Data resource, calculate the quilibrium constant K at 25.0°C for the following reaction. Fe2O3(s)+ 3H2(g)→ 2Fe(s)+ 3H2O(l) Round your answer to 2 significant digits. delta G of Fe2O3=-742.2 kj/mol h2=0 Fe=0 H20=-237.1kj/mol
Ff.137.
26) Suppose that at a pressure of 1 atm and temperature 300 K, a given material has two possible phases: liquid (L) and solid (S). We start the system with N₁ = 5 moles in the liquid phase and Ng = 9 moles in the solid phase. For these values of pressure and temperature, PL = 5 x 10-21 J • Hs9 x 10-21 J. What is the equilibrium value of NL? a. 9 mol b. 14 mol c. 1.49 mol d. 5 mol e. O mol
Consider the following equilibrium: 2NOC1 (g) → 2NO(g) + Cl₂ (g) AG = 41. kJ Now suppose a reaction vessel is filled with 8.30 atm of nitrosyl chloride (NOC1) and 5.80 atm of chlorine (C1₂) at 878. °C. Answer the following questions about this system: Under these conditions, will the pressure of Cl₂ tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of Cl₂ will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. оо rise fall yes no 0 atm x10 X Ś
#13 - Round your answer to 2 significant digits – as it states in the directions. If you do it correclty, I will give you a thumbs up!
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 50.0 L tank with 22. mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 6.6 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K-0 C = x10 X
Use the tabulated information to calculate the equilibrium constant (K) for for the following reaction, at 25°C. R= 8.314 J/mol.K 2HNO3(aq) + NO (g) → ) 3NO,(g) +H,O(l) NO (g) NO₂ (g) H₂O (1) AG() 87.6 51.3 -237.1 O 5.11 z 10-4 O 1.15 x 10-9 O 1.02 O 8.71 x 108 O 9.80 HNO3(aq) -110.9
Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant K at 25.0 °C for the following reaction. 2 NO (g) N2(g) + O2(g) Round your answer to 2 significant digits. K ☐ x10 ค
For the reaction 2 A(g) = B(g) + 3 C(g), we begin with only pure A(g) and the total pressure is 8.00 atm. We attain equilibrium. At equilibrium, the total pressure is 12.00 atm. What is the value of ∆G◦ for this reaction? The temperature is 25.0 ◦C throughout.
The steam reforming reaction of methane follows this chemical equation: CHA(g) + H50(g) - CO(g) + 3 H2(g) A H° = +193 kJ/mol At 298 K the reaction lies far to the reactant side with a very small equilibrium constant of 2.35 × 10-23. To obtain a significant amount of the desired hydrogen gas product, the reaction is operated at very high temperatures. What is the equilibrium constant at 1100 K?