Carbon reactswith water vapor at elevated temperatures.
Assuming a reaction mixture initially contains only reactants, what is the concentration of CO in an equilibrium mixture with [H2O] = 0.500M at 1000 °C?
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Chapter 13 Solutions
Chemistry Atoms First2e
- Phosphorus pentachloride, PCl5, decomposes on heating to give phosphorus trichloride, PCl5, and chlorine. PCl5(g)PCl3(g)+Cl2(g) A closed 2.90-L vessel initially contains 0.0564 mol PCl5. What is the total pressure at 250C when equilibrium is achieved? The value of Kc at 250C is 4.15 102.arrow_forwardNitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) Suppose you place 2.00 mol NOC1 in a 1.00–L flask, seal it, and raise the temperature to 462 °C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.arrow_forwardA mixture of carbon monoxide, hydrogen, and methanol, CH3OH, is at equilibrium according to the equation CO(g)+2H2(g)CH3OH(g) At 290C, the mixture is 0.034 M CO, 0.450 M H2, and 0.00023 M CH3OH. What is Kc for this reaction at 290C?arrow_forward
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- Suppose sulfur dioxide reacts with oxygen at 25C. 2SO2(g)+O2(g)2SO3(g) The equilibrium constant Kc equals 8.0 1035 at this temperature From the magnitude of Kc, do you think this reaction occurs to any great extent when equilibrium is reached at room temperature? If an equilibrium mixture is 1.0 M SO3 and has equal concentrations of SO2 and O2, what is the concentration of SO2 in the mixture? Does this result agree with what you expect from the magnitude of Kc?arrow_forwardAn experimenter places the following concentrations of gases in a closed container: [NOBr] = 7.13 102 M, [NO] = 1.58 102 M. [Br2] = 1.29 102 M. These gases then react: 2NOBr(g)2NO(g)+Br2(g) At the temperature of the reaction, the equilibrium constant Kc is 3.07 104. Calculate the reaction quotient, Qc, from the initial concentrations and determine whether the concentration of NOBr increases or decreases as the reaction approaches equilibrium. a Qc = 6.33 104; the concentration of NOBr decreases b Qc = 6.33 104; the concentration of NOBr increases c Qc = 1.58 104; the concentration of NOBr increases d Qc = 4.65 104; the concentration of NOBr decreases e Qc = 4.65 104; the concentration of NOBr increasesarrow_forwardAt high temperatures, a dynamic equilibrium exists between carbon monoxide, carbon dioxide, and solid carbon. C(s)+CO2(g)2CO(g);H=172.5kJ At 850C, Kc is 0.153. a What is the value of Kp? b If the original reaction system consisted of just carbon and 1.50 atm of CO2, what are the pressures of CO2 and CO when equilibrium has been established? c How will the equilibrium pressure of CO change if the temperature is decreased?arrow_forward
- Antimony(V) chloride. SbCl5, decomposes on heating to give antimony(III) chloride, SbCl3, and chlorine. SbCl5(g)SbCl3(g)+Cl2(g) A closed 3.50-L vessel initially contains 0.0125 mol SbCl5. What is the total pressure at 248C when equilibrium is achieved? The value of Kc at 248C is 2.50 102.arrow_forwardA 2.50-L vessel contains 1.75 mol N2, 1.75 mol H2, and 0.346 mol NH3. What is the direction of reaction (forward or reverse) needed to attain equilibrium at 401C? The equilibrium constant Kc for the reaction N2(g)+3H2(g)2NH3(g) is 0.50 at 401C.arrow_forwardFor the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.arrow_forward
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