Practice ProblemBUILD
The equation
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Connect 1-semester Access Card For Chemistry
- Solve all part please. Consider the equilibrium reaction N2O4 (g) ⇌ 2 NO2 (g)a. Using appendix C, find H and S for this reaction (you will need this for b,c). delta s= 176.6J delta H=5802kJb. Knowing that K is temperature dependent and that G = -RTlnK, find the equilibrium constant (K) and T whenthe above reaction is at equilibrium with PNO2 = PN2O4 = 1.0 atm.c. Knowing that K is temperature dependent and that G = -RTlnK, find the equilibrium constant (K) and T whenthe above reaction is at equilibrium with PT = 10.0 atm and PNO2 = 2 PN2O4.arrow_forwardAt a given temperature, the equilibrium constant (Kp) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.154. If 0.198 atm N2O4 is sealed in a flask, what partial pressure (in atm) of NO2 will exist at equilibrium? (no scientific notation)N2O4(g) ⇄ 2NO2(g)arrow_forwardA sample of SO3 decomposes according to the following equation: 2 SO3(g) 2 SO2(g) + 1 O2(g) An equilibrium mixture in a 10-L vessel at 645 oC, contains 0.0251 g of SO3, 0.0697 g of SO2, and 0.0185 g of O2. (a) Calculate KP for this reaction at this temperature. KP = . . (b) What is the total pressure exerted by the equilibrium mixture of gases? Ptotal = Incorrect: Your answer is incorrect. atm.arrow_forward
- Calculate K at 298 K for the following reaction: NO(g) + 1/2 O2 (g) <-> NO2 (g) Delta G (kJ/mol) for the following: NO(g) 86.60, NO2(g) 51, O2(g) 0 (answer in scientific notation)arrow_forwardCarbon monoxide and hydrogen react according to the following equation: CO (g) + H2 (g) CH4 (g) + H2O (g) When 1.00 mol of CO and 3.00 moles of H2 are placed in a 10.0 L container at 927 ° C (1200 K) and allowed to reach equilibrium, the mixture is found to have 0.363 moles of H2O What is the molar composition (that is, how many moles) of H2 are present in the equilibrium mixture? Answer:arrow_forwardThe reaction below has an equilibrium constant Kp=2.2×106 at 298 K. 2COF2(g)⇌CO2(g)+CF4(g). Calculate Kp for the reaction below. 4COF2(g)⇌2CO2(g)+2CF4(g)arrow_forward
- For the reaction: 2 A (g) + B (s) ⇌ 2 C (s) + D (g) Kp = 8210 At 298 K in a 10.0 L vessel, the known equilibrium values are as follows: 0.016 atm of A, 0.22 mol of B, and 10.5 mol of C. What is the equilibrium partial pressure of D? Answer ____ atmarrow_forwardConsider the following reaction: CO (g) + H2O (g) <===> CO2 (g) + H2 (g) a. Write the expression for the equilibrium constant (K) of the reaction b. Calculate the value for K using the following concentrations of each substance at equilibrium: [CO) = 0.55 M [H2O) = 0.44 M [CO2) = 0.25 M [H2) = 0.10 M c. Based on the value you obtained for K, are the products or reactants lower in energy? d. Is the value for ΔH negative or positive? please show workarrow_forward#7 Be sure to answer all parts. Calculate Kp for the following equilibrium: 3 O2(g) ⇌ 2 O3(g) Kc =1.8×10 −56 at 475 K Answer= ____x10____arrow_forward
- Gaseous hydrogen iodide is placed in a closed container at 425 ∘C ∘ C , where it partially decomposes to hydrogen and iodine: 2HI(g)←→H2(g)+I2(g) 2 H I ( g ) ← → H 2 ( g ) + I 2 ( g ) . At equilibrium it is found that [HI]= [ H I ] = 3.51×10−3 M M , [H2]= [ H 2 ] = 4.76×10−4 M M , and [I2]= [ I 2 ] What is the value of KcKc at this temperature? Please provide only typed answer solution no handwritten solution needed allowedarrow_forwardFor the reaction A (g) → 3 B (g), Kp = 0.241 at 298 K. What is the value of ∆G for this reaction at 298 K when the partial pressures of A and B are 5.70 atm and 0.250 atm? ∆G° = -RT ln K. Since K is not provided, try using the partial pressures in its place.arrow_forwardissue 6Choose the equilibrium in which the products are favored by a drop in pressure and the reactants favored by a drop in temperature.a) N2(g) + 3 H2(g) ⇔ 2 NH3(g) + 92.3 kJb) H2(g) + I2(g) + 51.8 kJ ⇔ 2 HI(g)c) PCl3(g) + Cl2(g) ⇔ PCl5(g) ΔH = -84.2 kJd) 2 NO2(g) ⇔ 2 NO(g) + O2(g) ΔH = +54 kJarrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY