In the lower atmosphere, oxygen is converted to ozone
For each of the following changes at equilibrium, indicate whether the equilibrium shifts in the direction of product, reactants, or does not change:
a. adding more
b. adding more
c. increasing the temperature
d. increasing the volume of the container
e. adding a catalyst
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Basic Chemistry
- . Consider an equilibrium mixture consisting of H2O(g), CO(g). H2(g), and CO2(g) reacting in a closed vessel according to the equation H2O(g)+CO(g)H2(g)+CO2(g)a. You add more H2O to the flask. How does the new equilibrium concentration of each chemical compare to its origin al equilibrium concentration after equilibrium is re-established? Justify your answer. b. You add more H2to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.arrow_forwardConsider the equilibrium FeO(s)+CO(g)Fe(s)+CO2(g) When carbon dioxide is removed from the equilibrium mixture (say, by passing the gases through water to absorb CO2), what is the direction of net reaction as the new equilibrium is achieved?arrow_forwardA chemist put 1.18 mol of substance A and 2.85 mol of substance B into a 10.0-L flask, which she then closed. A and B react by the following equation: A(g)+2B(g)3C(g)+D(g) She found that the equilibrium mixture at 25C contained 0.376 mol of D. How many moles of B are in the flask at equilibrium at 25C? a 2.47 mol b 3.60 mol c 2.52 mol d 2.10 mol e 2.41 molarrow_forward
- Phosphorus pentachloride decomposes at elevated temperatures. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 3.120 g of PCl5, 3.845 g of PCl3, and 1.787 g of Cl2 in a 10.0-L flask. If you add 1.418 g of Cl2, how will the equilibrium be affected? What will the concentrations of PCl5, PCl3, and Cl2 be when equilibrium is reestablished?arrow_forwardConsider the following hypothetical dissociation: AB3(s) A3+(aq)+3 B(aq)H0What effect will each of the following have on the position of equilibrium? (a) addition of A(NO3)3 (b) increase in temperature (c) adding Na+, forming NaBarrow_forwardConsider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.arrow_forward
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- Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon. (a) Write the expression for the equilibrium constant for the reversible reaction C(s)+H2O(g)CO(g)+H2(g)H=131.30kJ (b) What will happen to the concentration of each reactant and product at equilibrium if more C is added? (c) What will happen to the concentration of each reactant and product at equilibrium if H2O is removed? (d) What will happen to the concentration of each reactant and product at equilibrium if CO is added? (e) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?arrow_forwardHeating a metal carbonate leads to decomposition. BaCO3(s) BaO(s) + CO2(g) Predict the effect on the equilibrium of each change listed below. Answer by choosing (i) no change, (ii) shifts left or (iii) shifts right. (a) add BaCO3 (b) add CO2 (c) add BaO (d) raise the temperature (e) increase the volume of the flask containing the reactionarrow_forwardA necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide. SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO3 is lower than it would be at lower temperatures. 2SO2(g)+O2(g)2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic?arrow_forward
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