7.8 When 0.210 moles of Br2 are placed into a sealed 0.800 dm³ flask at 1500 °C1.5% of the molecules dissociate. noBr2(g)prob2Br(g)a) Calculate the value of Kc at this temperature.b) What value of Kc do you expect if the total pressure of the system is doubled?250 dm3 was filled with 5.00 moles of NOCI and

Step 1: First let's calculate the dissociated moles of Br2:dissociated=(0.210mole…

Answered: 7.8 When 0.210 moles of Br2 are placed…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 36QAP: At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s),...

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At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
Hemoglobin (Hb) binds to both oxygen and carbon monoxide. When the carbon monoxide replaces the oxygen in an organism, the following reaction occurs: HbO2(aq)+CO(g)HbCO(aq)+O2(g) At 37C, K is about 200. When equal concentrations of HbO2 and HbCO are present, the effect of CO inhalation is fatal. Assuming PO2=0.21atm, what is PCO when [ HbO2 ]=[ HbCO ]?
The reaction NO (g) « N2 (g) + O2 (g) has a value of KC = 2400 at a temperature of2000 K. If 0.61 g of NO are put in a previously empty 3.00 L vessel, calculate the equilibriumconcentrations of NO, N2, O2. What can be said regarding the result?
Be sure to answer all parts. In the lower troposphere, ozone is one of the components of photochemical smog. It is generated in air when nitrogen dioxide, formed by the oxidation of nitrogen monoxide from car exhaust, reacts by the following mechanism: (1) NO2(g) NO(g) + O(g) (2) O(g) + 02(g) , 03(g) where k = 6.0 x 103s; k2 = 1.0 x 10° L/mol s; [NO2] = 4.0 x 10- M; and [O2] = 3.0 x 102 M. Assuming the rate of formation of atomic oxygen in step 1 equals the rate of its consumption in step 2, calculate the concentration of atomic oxygen [0]. Enter your answer in scientific notation. x 10 (select) M
The reaction: 2SO₂(g) + O₂(g) = 2SO3(g) has an equilibrium constant, Kc = 4.4 Suppose a mixture contains 0.22 M SO₂, 0.16 M O2, and 0.25 M SO3. Calculate the value of Qc and predict whether the system is at equilibrium or not at equilibrium. If not at equilibrium, indicate the direction of net reaction. (A) Qc = 0.12; system is not at equilibrium; a net forward reaction occurs to form more SO3 (B) Qc = 7.1; system is not at equilibrium; a net forward reaction occurs to form more SO3 (C) Q = 8.1; system is not at equilibrium; a net back reaction occurs to form more SO₂ and 0₂ (D) Qc = 4.4; system is at equilibrium and there is no net reaction
Consider the rxn A(g) <--> 2B(g) where Kc =1.5 at 298 K. If 3.0 moles of A and 3.0 moles of B are introduced into a 1.00 liter flask at 298 K, what change in concentrations (if any) would occur in time? Does A increase, decrease, or stay the same? Does B increase, decrease, or stay the same?
Consider the following equilibrium: C,H6(g) + C3H12(g) = CH4(g) + C,H14(g); Kp = 9.57 at 500 K Suppose 13.3 g each of CH4 (MW= 16), C2H6 (MW = 30), C3H12 (MW = %3D 72), and CGH14 (MW = 86) are placed in a 50.0-L reaction vessel at 500 K. What is the value of Q,?
Would you increase or decrease the pressure (via a volume change) of each of the following reaction mixtures to decrease the yield of products? (a) 2SO2(g) + O2(g) (b) 4NH3(g) + 502(g) = 4NO(g) + 6H20(g) (c) CaC,04(s) = CaCO3(s) + CO(g) = 2S03(g) O (a) increase P; (b) increase P; (c) decreases P O (a) decrease P; (b) increase P; (c) decrease P O (a) decrease P; (b) increases P; (c) increase P O (a) increase P; (b) increases P; (c) increase P
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The equilibrium concentration of the gases at 1500 K are [BrF5] = 0.0064 mol dm-3, [Br2] = 0.0018 mol dm-3 and [F2] = 0.0090 mol dm-3 . Calculate the value of Kc at this temperature.
A student ran the following reaction in the laboratory at 1090 K: 2s0,(2) + O,(g)=2s03(g) When he introduced so,(g) and O2(g) into a 1.00 L evacuated container, so that the initial partial pressure of SO2 was 4.66 atm and the initial partial pressure of O, was 1.51 atm, he found that the equilibrium partial pressure of O2 was 0.504 atm. Calculate the equilibrium constant, K: she obtained for this reaction. Kp =|
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