1) The equation for the formation of hydrogen iodide from H; and I, is:Halg)+ 12(g) 2HI(g)The value of K, for the reaction is 91.0 at 955 °C. What is the equilibrium partialpressure of HI in a sealed reaction vessel at 955 °C if the initial partial pressuresof H, and I, are both 0.100 atm and initially there is no HI present?2

Answered: Image /qna-images/answer/2575e42d-4518-4150-96cd-6176578a8e14.jpg

Answered: 1) The equation for the formation of…

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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Hydrogen iodide gas is formed from its elements with a value for Kp = 25.5 at a certain temperature: H2 (g) + I2 (g) <---> 2 HI (g) What will the equilibrium pressure (in atm) of hydrogen iodide gas be if the initial partial pressure of both reactant gases is 0.150 atm?
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K.H2 (g) + I2 (g) 2 HI (g)Calculate the equilibrium concentrations of reactants and product when 0.228 moles of H2 and 0.228 moles of I2 are introduced into a 1.00 L vessel at 698 K. [ H2 ] = M [ I2 ] = M [ HI ] = M
The equilibrium constant (Kc ) for the reaction: PCl3 + Cl2 <=> PCl5 equals 51 at 235°C. If 0.648 mol of phosphorus trichloride and 0.748 mol chlorine (Cl2) are added to a 9.00 L reaction vessel, what is the amount of moles of Cl2 at equilibrium in the mixture at 235°C?
The equilibrium constant, K, for the following reaction is 1.47×10-2 at 308 K. NH4HS(s) NH3(g) + H2S(g) An equilibrium mixture in a 15.3 L container at 308 K contains 0.247 mol NH4HS(s), 0.159 M NH3 and 9.25×10-2 M H2S. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 8.49 L? [NH3] = M [H2S] = M
Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures, according to the following reaction. N2(g) + O2(g) ⇌ 2 NO(g) The equilibrium constant for the reaction is KP = 0.233 at 1840 ℃. If a container is charged with 0.403 atm of nitrogen and 0.300 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen? Report your answer to THREE significant figures.
The equilibrium constant Kp for the reaction,2 SO3(g) <-------> 2 SO2(g) + O2(g)is 7.880 at 759 °C. If a vessel at this temperature initially contains pure SO3 and if the partial pressure of SO3 at equilibrium is 0.109 atm, what is the partial pressure of O2 in the flask at equilibrium? What was the initial pressure of SO3 in the flask?
At 400°C the reaction BaO2(s) + 4 HCI(g) 2 BaCl,(s) + 2 H,O(g) + Cl2(g) has an equilibrium constant equal to K1. How is K¡ related to the equilibrium constant K, of the reaction 2 Cl2(g) + 4 H,O(g) + 2 BaCl2(s) 2 8 HCl(g) + 2 BaO2(s) at 400°C?
At a given temperature, the equilibrium constant K, for the reaction below is 2.68×10¯³. 2s0,(g) +02(g) 2so, (g) What is the value of the equilibrium constant for each of the following reactions at that temperature? so,) + 0,) – so,() 250, (2). - 250, (g) + 0,(g) so, )
At 900 K, the following reaction has Kp = 0.345: 2 SO2(g) + O2(g) ⇋ 2 SO3(g). In an equilibrium mixture, the partial pressure of SO2 and O2 are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3 in the mixture?
A chem ngineer is studying the following reaction: 4 HCl(g)+O,(g) – 2 H,0(g)+2Cl,(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.0040. The engineer charges ("fillsf) four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. He then measures the co mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound pressure expected change in pressure vessel HCl 8.71 atm Ot increase O! decrease O (no change) 02 8.13 atm O t increase OI decrease O (no change) H,0 3.63 atm Ot increase OI decrease (no change) I decrease (no change) Cl, 1.91 atm ease I decrease (no change) 7,61 atm t increase HCI I decrease O (no change) 7,86 atm O f increase 0, I decrease O (no change) 4.18 atm t increase H,0 I decrease (no change) t increase 2.46 atm Cl, I decrease O (no…
Write equilibrium-constant expressions K, for each of the following reactions. PC|3(g) + 3NH3(g) D P(NH2)3g) + 3HC((g) 4NH3(g) + 502E)D 4NO(g) + 6H20(g) NazCO3(s) + SO23) + ½ O2(g) D Naz504(s) + CO2(g)
What is the value of the equilibrium constant Kc of the reaction at the temperature of the vessel?

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