Nitrous oxide, N₂O, is a gas used as an anesthetic; it is sometimes called "laughing gas." This compound has a strong tendency todecompose into nitrogen and oxygen following the equation:2N2O(g) 2N2(g) + O2(g)But the reaction is so slow that the gas appears to be stable at room temperature (33 °C). The decomposition reaction has K= 1.3E+34.What is the value of Kp for this reaction at 33 °C? (Express your answer in scientific notation.)Kp= i

Given: T=33°C2N2O(g)⇌2N2(g)+O2(g)Kc=1.3x1034Step 1: Write the formula we need to…

Answered: Nitrous oxide, N₂O, is a gas used as an…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 104AP: . The reaction PCl3(l)+Cl2(g)PCl5(s)liberates 124 kJ of energy per mole of PCl3reacted. Will an...

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12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.
Given these data at a certain temperature, 2H2(g)+O2(g)2H2O(g)Kc=3.21081N2(g)+3H2(g)2NH3(g)Kc=3.5108 calculate Kc for the reaction of ammonia with oxygen to give N2(g) and H2O(g).
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Consider the following relationships: G = 1, H = TS, Q = 1. G = G, K = 1 Which of these relationships is(are) always true for a reaction at equilibrium?
The equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at 250C and 1.8 at 275C. Is this reaction endothermic or exothermic?
Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are placed in a closed 10.0-L vessel, what is the mole fraction of HI in the mixture when equilibrium is reached at 205C? Use data from Appendix C and any reasonable approximations to obtain K.
12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant into a lake and estimates that this may warm the water locally to 25 °C. One question to be considered is the effect of this temperature change on the uptake of CO2 by the water. The equilibrium constant for the reaction CO2+H2OH2CO3 ; is K=1.7103 at 25 °C. Because bonds form, the reaction is exothermic. (a) Will this reaction progress further toward products at higher temperatures near the water discharge with its warmer water than it would in the cooler lake water? Explain your reasoning. (b) Carbonic acid has a Kaof 2.5104 at 25 °C. What is the equilibrium constant for the CO2+2H2OHCO3+H3O+? (c) What additional factor should the engineer be considering about CO2 gas, probably before considering this reaction chemistry?
Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated with oxides as a catalyst. For the reaction N2(g)+3H2(g)2NH3(g) equilibrium constants (Kp values) as a function of temperature are 300C, 4.34 103 500C, 1.45 105 600C, 2.25 106 Is the reaction exothermic or endothermic?
Consider the following equilibria involving SO2(g) and their corresponding equilibrium constants. SO2(g) + 12 O2(g) SO3(g) K1 2SO3(g) 2SO2(g) + O2(g) K2 Which of the following expressions relates K1 to K2? (a) K2=K12 (b) K22=K1 (c) K2 = K1 (d) K2 = 1/K1 (e) K2=1/K12
Limestone decomposes at high temperatures. CaCO3(s) CaO(s) + CO2(g) At 1000 C, Kp = 3.87. If pure CaCO3 is placed in a 5.00-L flask and heated to 1000 C, what quantity of CaCO3 must decompose to achieve the equilibrium pressure of CO2?
. Plants synthesize the sugar dextrose according to the following reaction by absorbing radiant energy from the sun (photosynthesis). 6CO2(g)+6H2O(g)C6H12O6(g)+6O2(g)Will an increase in temperature tend to favor or discourage the production of C6H12O6(s)?
One way of preparing hydrogen is by the decomposition of water. 2H2O(g)2H2(g)+O2(g);H=484kJ Would you expect the decomposition to be favorable at high or low temperature? Explain.

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