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Hydrogen peroxide, H2O2, is used to disinfect contact lenses. How many milliliters of O2(g) at 22 °C and 1.00 bar can be liberated from 10.0 mL of an aqueous solution containing 3.00% H2O2 by mass? The density of the aqueous solution of H2O2 is 1.01 g/mL.
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Chapter 6 Solutions
General Chemistry: Principles And Modern Applications Plus Mastering Chemistry With Pearson Etext -- Access Card Package (11th Edition)
- Which of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substancearrow_forward6. When the ideal-gas reaction A+B=C+Dhas reached equilibrium, state whether or not each of the following relations must be true. Here n¡ is the number of moles of species i in equilibrium, P, is the partial pressure of i, and µ; is the chemical potential of i. Here a simple True or False answer is sufficient. (a) nc+np=nA +ng (b) Pc+Pp=PA+PB (c) na=ng (d) nc=na (e) If only A and B are present initially, then nc=np (f) Ha + HB= Hc+ Hp no matter what the initial composition. (g) If only A and B are present initially, then in equilibrium we must have nc # 0. (h) The equilibrium constant Kp(T)= PĄPB/(PcPp). (i) The value of –RT In Kp(T) = µE(T)+µ8(T)– H3(T) –- H§(T). ) The equilibrium constant is independent of the total pressure.arrow_forwardCalculate the value of the equilibrium constant, Ke, for the reaction Q(g) + X(g) 2 M(g) + N(g) given that Ke = M(g) = Z(g) 6R(g) = 2N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) .116 Kel = 3.57 Kc2 = 0.524 Kc3 = 14.6arrow_forward
- The equilibrium constant Kc for the reaction N2(g) + O2(g)⇋ 2NO(g) at 1200 degrees Celsius is 1.00 x 10-5. Calculate the equilibrium molar concentrations of NO, N2, O2 in a reaction vessel of volume 10.00 L that initially held 0.312 mol N2 and 0.407 mol O2.arrow_forwardWrite the formula for hypoiodous acid. formula: || SPECIAL ΔΣΩ λμπ x" Xo x (s) (1) (aq) (g) () [] CLRarrow_forwardThe emission of NO, by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea reduces NO (which oxidizes in air to form NO2) according to the reaction: 2 CO(NH;)»(3) + 4 NO(3) + O2(8) 4 Na(8) + 2 CO;(g) + 4 H¿O(g) Suppose that the exhaust stream of an automobile has a flow rate of 2.55 L/s at 655 Kand contains a partial pressure of NO of 12.4 torr. What total mass of urea is necessary to react complete- ly with the NO formed during 8.0 hours of driving?arrow_forward
- Calculate the value of the equilibrium constant, Kc, for the reaction Q(g) + X(g) 2 M(g) + N(g) given that Kc = M(g) = Z(g) 6R(g) — 2N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kc1 = 3.01 Kc2 = 0.433 Kc3 = 12.5arrow_forward4) a) A reaction chamber is divided into two sections by a partition on which a valve is inserted. One section contains pure gas A and the other section has a mixture of gases A and B. What happens when the valve is opened? Explain this process in terms of chemical potential. b) The decomposition of etane into etene and hydrogen takes places at 1000 K and under 1 bar total pressure. C,H6(g) → C2H48) + H2«g) The composition of the mixture at equilibrium is as follows : H2(g): 32, C2H4(g): 32, and C,H6(g):36 (mol, %). According to the data; Calculate K, at 1000K Calculate Kp at 298.15 K, AH° = 145 kJ/mol Calculate AG° at 298.15 Karrow_forwardb) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction СO(g) +2H2(g) — CHОН (g) At 298.15 K, AH.co (0)= -26.41 kcal/mol, AH AG.co (9)= -32.8079 kcal/mol, AG cH,oh(9)= -38.69 kcal/mol, °.CH20H(9)= -48.08 kcal/mol, The standard heat capacity of various components is given by, CO = a + bT + cT² + dT³, where C, is in cal/mol-K and T is in K b x10² с х105 d x10° Соmponent CH3OH а 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079arrow_forward
- A 23.9 g sample of nitrogen monoxide is injected into a 3.17–L reaction vessel that contains 28.2 g of nitrosyl bromide. When the system comes to equilibrium at 133 ℃, what is the total pressure inside the reaction vessel? The equilibrium constant, KC = 0.0205 at this temperature. R = 0.082058 L⋅atm/mol⋅K. Report your answer to THREE significant figures. 2 NO(g) + Br2(g) ⇌ 2 NOBr(g)arrow_forwardWrite an expression for the equilibrium constant for this reaction: N2O4(g)+ O3(g)=N2O5(s)+O2(g)arrow_forwardGiven the reaction: 2 B(s) + 3 H2(g) ↽−−⇀ 2 BH3(g) at 25 oC. At equilibrium, 0.254 moles BH3, 0.588 moles H2 and 0.666 mole B are found in a 1.0 L flask. Determine the value of Kc. Express the answer to 3 sig. figs.arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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