Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Consider the following reaction: SO₂Cl2 (g) SO₂ (g) + Cl₂ (g) A reaction mixture is made containing an initial [SO₂Cl₂] of 2.4×10-2 M. At equilibrium, [Cl₂] = 1.3×10-² M. Part A Calculate the value of the equilibrium constant (Kc). Express your answer to two significant figures.arrow_forwardHydrogen and chlorine react to form hydrogen chloride, like this: H,(g) + Cl,(g) 2 HCl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chloride has the following composition: compound concentration at equilibrium 0.86 M Cl, 0.30 M HC1 1.9 M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0arrow_forwardQ2 For the chemical reaction shown below select the correct the equilibrium constant expression for 4NH3(g) + 302(g) = 2N2(9) + 6H2O(g) Q3 4NH3(9) + 302(9) = 2N2(9) + 6H2O(9) If a chemist mixed 2.930 moles of ammonia (NH3) gas with 1.978 moles of oxygen (02) gas in a 7.95 Liter air tight metal flask at 127°C and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas then how many moles of ammonia (NH3) is present at equilibrium? 4NH3(9) + 302(9) 2N2(9) + 6H2O(g) Q4 If a chemist mixed 2.930 moles of ammonia (NH3) gas with 1.978 moles of oxygen (02) gas in a 7.95 Liter air tight metal flask at 127°C and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas then how many moles of water (H,O) is present at equilibrium? 4NH3(9) + 302(g) 2N2(9) + 6H2O(9) Q5 If a chemist mixed 2.930 moles of ammonia (NH3) gas with 1.978 moles of oxygen (02) gas in a 7.95 Liter air…arrow_forward
- Part A For the reaction 3H2 (g) + N2 (g) = 2NH3 (g) at 225 °C the equilibrium contant is 1.7 × 102. If the equilibrium mixture contains 0.13 M H2 and 0.018 M N2 , what is the molar concentration of NH3 ? Express your answer to two significant figures and include the appropriate units.arrow_forwardCalculate the equilibrium concentrations for each reactant and product in the following equation at initial concentrations of 0.0400 M SO2, 0.0500 M NO2, 1.300 M NO and 0.200 M SO3. The equilibrium constant for this reaction, Kc = 85.0. SO2(g) + NO2(g) ↔ NO(g) + SO3(g) Group of answer choices [SO2] = 0.0275, [NO2] = 0.0375, [NO] = 1.313, [SO3] = 0.213 [SO2] = 0.0309, [NO2] = 0.0409, [NO] = 1.309, [SO3] = 0.209 [SO2] = 0.0525, [NO2] = 0.0625, [NO] = 1.288, [SO3] = 0.188 [SO2] = 0.0491, [NO2] = 0.0591, [NO] = 1.291, [SO3] = 0.191arrow_forwardFor the reaction below, the concentrations at equilibrium are [SO₂] = 0.60 M, [O₂] = 0.25 M, and [SO₂] = 1.6 M. What is the value of the equilibrium constant, Ke? 2 SO₂(g) + O₂(g) →→→ 2 SO₂(g) • Report your answer using two significant figures. Provide your answer below:arrow_forward
- The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K.NH4Cl(s) NH3(g) + HCl(g)If an equilibrium mixture of the three compounds in a 5.01 L container at 548 K contains 2.51 mol of NH4Cl(s) and 0.217 mol of NH3, the number of moles of HCl present is _____ moles.arrow_forwardWrite the equilibrium constant expression, K , for the following reaction: (If either the numerator or denominator is blank, please enter 1.) K=arrow_forward1.arrow_forward
- Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)→2 HgO(s) At a certain temperature, a chemist finds that a 7.0 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 7.0 g O2 5.8 g HgO 16.5 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = | x10arrow_forwardThe following reaction has an equilibrium constant of 2.65 x10-3 at 300K. Br2 (g) + Cl2 (g) 2 BrCl (g) Which of the following statements is true? Question 5 options: The system has a higher concentration of reactant molecules than product molecules at equilibrium, but there are significant quantities of both. The system consists almost entirely of reactant molecules at equilibrium. The system consists almost entirely of product molecules at equilibrium. The system has approximately equal concentrations of product and reactant molecules at equilibrium. The system has higher concentrations of product molecules than reactant molecules at equilibrium, but there are significant quantities of both.arrow_forwardNitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(g) + H₂O(1)→2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 3.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound NO₂ H₂O HNO3 NO amount 5.9 g 142.0 g 15.1 g 12.0 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. с K = D 0 C x10 X Śarrow_forward
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