Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200. mL flask with 4.8 atm ofammonia gas, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 4.3 atm.Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.K-1P=x10×G

Kp = 31. Explanation:Step 1Given , Initial pressure of NH3 = 4.8 atm equilibrium pressure of H2 =…

Answered: Ammonia will decompose into nitrogen…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 10QRT

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Calculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and H2O() in a reaction at constant pressure and 298.15 K.
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-.
Write a balanced chemical equation for a totally gaseous equilibrium system that would lead to the following equilibrium constant expression. Keq=[N2]2[H2O]6[NH3]4[O2]3
Indicate which of the following processes are reversible. (a) Nitrogen gas expands into a vacuum. (b) Dry ice, CO2(s), sublimes at 25 C and 1.0 atm. (c) Energy as heat is added to a mixture of ice and water at 0 C, causing some of the ice to melt. (d) Methanol and ethanol mix forming a homogeneous solution.
When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200. °C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. Write a balanced chemical equation for the equilibrium reaction. Use bond enthalpies from Table 6.2 ( Sec. 6-6b) to estimate the enthalpy change for the reaction. Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? In which direction will the equilibrium shift as the temperature increases above 200. °C? Explain. Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? Why is the equilibrium not established at room temperature?
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
The hydrocarbon naphthalene was frequently used in mothballs until recently, when it was discovered that human inhalation of naphthalene vapors can lead to hemolytic anemia. Naphthalene is 93.71% carbon by mass, and a 0.256-mole sample of naphthalene has a mass of 32.8 g. What is the molecular formula of naphthalene? This compound works as a pesticide in mothballs by. sublimation of the .solid so that it fumigates enclosed spaces with its vapors according to the equation Naphthalene(s)naphthalene(g)K=4.29106(at298K) If 3.00 g solid naphthalene is placed into an enclosed space with a volume of 5.00 L at 25C, what percentage of the naphthalene will have sublimed once equilibrium bas been established?
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.

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