For the reaction below, formation salpies at 1 bar and standart entropies are given. Çe te equilibrium constant (Kp) of the reaction at 580 K. X(g) +3 Y,(g) =2XY,(g) For X,(g) AHº,f =0 kJ mol S° = 179 J mol* K For Y(g) AH°f = 0kJ mol* S° = 215 J mol"K** For XY,(g) AH°f = -146 kJ mol" S° = 154 mol K* R = 0.08206 L atm mol-1 K-1 = 8.314 J mol-1 K-1

For the reaction below, formation salpies at 1 bar and standart entropies are given. Çe te equilibrium constant (Kp) of the reaction at 580 K. X(g) +3 Y,(g) =2XY,(g) For X,(g) AHº,f =0 kJ mol S° = 179 J mol* K For Y(g) AH°f = 0kJ mol* S° = 215 J mol"K** For XY,(g) AH°f = -146 kJ mol" S° = 154 mol K* R = 0.08206 L atm mol-1 K-1 = 8.314 J mol-1 K-1

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 105QRT

See similar textbooks

Similar questions

Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Suppose you have an exothermic reaction with H = 15 kJ and a S of +150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.
The value of delta G at 281.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) + 3CI2 (g) ---> 2PCI3 (g) is _____ kJ/mol. At 25.0oC for this reaction delta H is -720.5kJ/mol, delta G is -642.9 kJ/mol, and delta S is -263.7 J/K.
For a new reaction A + B ----->C, an equilibrium constant of 2.4x106 was obtained at 300 K. In a separate calorimetry experiment, also at 300 K, the enthalpy was found to be 34 kJ/mole. What would the equilibrium constant be at 420 K?
Calculate the equilibrium constant, Kp at 1300 ℃ for the reaction shown below if the standard enthalpy of reaction, ΔH°rxn = −42.0 kJ/mol at 126 ℃ and the equilibrium constant at this temperature is Kp = 21.3. CO(g) + Br2(g) ⇌ COBr2(g), ΔH = −42.0 kJ/mol R = 8.314472 J/mol⋅K. Report your answer to THREE significant figures. Enter your answer in the appropriate boxes and remember a number such as 1.23 is 1.23 × 100 in scientific notation. Note: Your answer is assumed to be reduced to the highest power possible.
10.0 mol PCl3(g), 20.0 mol Cl2(g), and 40.0 mol PCl5(g) are introduced in a previously evacuated 10.0-L vessel at 25.0oC. The KP for the reaction at this temperature is 1.47×10–7: PCl5(g) →← PCl3(g) + Cl2(g), KP= 1.47×10–7 What is the immediate Gibbs free energy change for the reaction? In what direction the reaction will spontaneously approach equilibrium? Enter your answer with correct units and significant figures, and check the correct box below: Reaction proceeds spontaneously forward towards equilibrium. Reaction is at equilibrium. Reaction proceeds spontaneously backward towards equilibrium.
For a particular reaction, the equilibrium constant at 25 Celsius is known to be 1254. If the standard chnage in enthalpy for the reaction is -32 kJ/mol. What willl be tthe equilibrium constant at 37 Celsius?
(Q77) The standard Gibbs free energy (∆G°rxn) for the formation of sulfur trioxide from sulfur dioxide and oxygen gas is -72.3 kJ/mol. The balanced chemical equation is SO2 (g) + ½ O2 (g) --> SO3 (g). What will be the Gibbs Free energy of the reaction (in kJ/mol) if it takes place at a low temperature of -24.6 and the concentrations of three gases are: SO2 = 0.174 M O2 = 0.167 M SO3 = 1.32 M (One decimal place)
Calculate the equilibrium constant, Kp at 640 ℃ for the reaction shown below if the standard enthalpy of reaction, ΔH°rxn = −28.0 kJ/mol at 124 ℃ and the equilibrium constant at this temperature is Kp = 30.1. CO(g) + Br2(g) ⇌ COBr2(g), ΔH = −28.0 kJ/mol R = 8.314472 J/mol⋅K. Report your answer to THREE significant figures. Enter your answer in the appropriate boxes and remember a number such as 1.23 is 1.23 × 100 in scientific notation.
. Find the maximum possible temperature that may bereached when 0.050 mol Ca(OH)2(s) is allowed to reactwith 1.0 L of a 1.0-M HCl solution, both initially at 25°C.Assume that the final volume of the solution is 1.0 L, andthat the specific heat at constant pressure of the solutionis constant and equal to that of water, 4.18 J K-1g-1.
The standard heat of formation for Ag2CrO4(s) is -712 kJ/mol at 298 K. Write the formation equation for Ag2CrO4(s) that goes with this value of ΔH°.Be sure to specify states. Write fractions with a slash, such as 1/2 for one half.