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Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

SectionU6.5: How Balanced: Equilibrium Calculations

Problem 1TAI

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At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
5.49. Consider the following equilibrium: What is the effect on the equilibrium of each of the following changes? (You may need to calculate some standard enthalpy or Gibbs energy changes to answer these.) (a) The pressure is increased by decreasing the volume. (b) The temperature is decreased. (c) The pressure is increased by the addition of nitrogen gas, .
Explain the Criterion for chemical equilibrium for a fixed mass at a specified temperature and pressure ?
A mixture of 1.00 mol NaHCO;(s) and 1.00 mol Na,CO3(s) is introduced into a 2.50 L flask in which the partial presure of CO, is 2.10 atm and that of H,O (g) is 715 mmHg. When equilibrium is established at 100°C, will the partial pressures of CO(g) and H,0(g) be greater or less than their initial partial pressures? Explain. 2 NaHCO3(s) = Na2CO3(s) + CO2{g) + H2O(g) Kp = 0.23 at 100 °C
Chlorine and water react to form hydrogen chloride and oxygen, like this: 2 Cl,(g)+2H,0(g)-4 HCl(g)+O,(g) Write the pressure equilibrium constant expression for this reaction.
In a 3.0 L vessel the following equilibrium partial pressure are measured: N2= 90 torr, H2= 317 torr, NH3=1.00 x10^3 torr N2 (g) + 3H2 (g) -> 2NH3 (g) if hydrogen is removed from the vessel until the partial pressure of nitrogen, at equilibrium, is 250 torr. Calculate the partial pressure of the other substances under the new conditions. (Use the numbers at the top to find kp, then make those equilibrium conditions initial conditions to figure out this last part. The change in nitrogen will allow you (through stoich) to find the change in ammonia. The you can use Kp to find the partial pressure of hydrogen).
Suppose 1.000 mol CO and 3.000 mol H2 are put in a 10.00 L vessel at 1200 K. The equilibrium constant for Kc for CO(g) + 3H2(g) > CH4 (g) + H2O (g) is equal 3.92. find the equilibrium composition of the reaction mixture.
Bromine monochloride is synthesized using the reaction Br, (g) + Cl, (g) = 2BrCl(g) Кр 1.1 x 10-4 at 150 K A 206.0 L flask initially contains 0.965 kg of Br, and 1.012 kg of Cl,. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: g What is the percent yield of BrCl? percent yield:
Suppose 1.000 mol CÓ and 3.000 mol H2 are put in a 10.00 L vessel at 1200 K. The equilibrium constant for K, for CO(g) + 3H,(g) CH,(g) + H,O(g) equals 3.92. Find the equilibrium composition of the reaction mixture.
Suppose 1.000 mol CO and 3.000 mol H2 are putted in a 1.00 L vessel at 1200 k. The equilibrium constant for kc for reverse reaction of CO(g) + 3H2(g) produces CH4(g) + H2O(g) is equals 3.92. find the equilibrium composition of the mixture

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Is there a pattern to change in pressure, amount, K, pH?