In the ideal gas experiment, the students forgot to record the equilibrium temperature after reacting the magnesium ribbon to the acid. For their calculations, they assumed this temperature to be 25 °C. If the actual temperature was 28 °C, how will this affect the value of the calculated moles of gas produced? a. Indeterminate b. Increase C. No effect O d. Decrease

In the ideal gas experiment, the students forgot to record the equilibrium temperature after reacting the magnesium ribbon to the acid. For their calculations, they assumed this temperature to be 25 °C. If the actual temperature was 28 °C, how will this affect the value of the calculated moles of gas produced? a. Indeterminate b. Increase C. No effect O d. Decrease

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 109CP: A 1.604-g sample of methane (CH4) gas and 6.400 g oxygen gas are scaled into a 2.50-L vessel at 411C...

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A 1.604-g sample of methane (CH4) gas and 6.400 g oxygen gas are scaled into a 2.50-L vessel at 411C and are allowed to reach equilibrium. Methane can react with oxygen to form gaseous carbon dioxide and water vapor, or methane can react with oxygen to form gaseous carbon monoxide and water vapor. At equilibrium. the pressure of oxygen is 0.326 atm, and the pressure of water vapor is 4.45 atm. Calculate the pressures of carbon monoxide and carbon dioxide present at equilibrium.
. For an equilibrium involving gaseous substances, what effect, in general terms, is realized when the volume of the system is decreased?
. Consider the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the following changes affect the number of moles of each component of the system after equilibrium is re-established by completing the table. Complete the table with the terms increase, decrease, or no change. N2 H2 NH3 Add N2(g) Remove H2(g) Add NH3(g) Add Ne(g) (constant V) Increase the temperature Decrease the volume (constant T) Add a catalyst
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
Suppose you have two identical unopened bottles of carbonated beverage. The contents of both bottles appear to be perfectly clear. You loosen the cap of one of the bottles and hear a hiss as gas escapes, and at the same time gas bubbles appear in the liquid. The liquid in the unopened bottle still appears to be perfectly clear. Explain these observations using the concept of equilibrium and Le Chteliers principle. Remember, a carbonated beverage contains carbon dioxide gas dissolved in a liquid under pressure.
At 600C, gaseous CO and Cl2 are mixed together in a closed container. At the instant they are mixed, their concentrations are CO=0.79mol/L and Cl2=0.69mol/L. After equilibrium is established, their concentrations are CO=0.25mol/L and Cl2=0.15mol/L. Evaluate the equilibrium constant for the reaction CO(g)+Cl2(g)COCl2(g)
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.
. Suppose are action has the equilibrium constant K=1.3108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
Colorless hydrogen gas (H2) and red-brown colored bromine gas (Br2) reacts to form colorless HBr gas. Describe how the concentrations of H2, Br2, and HBr would change increase or decrease as equilibrium was established in a sealed container that initially contained only H2 and Br2. What observation would indicate that equilibrium had been established?
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.