I Review | Const Consider the reaction and its equilibrium constant: N204(g) = 2NO2(g) Ke = 5.85 x 10 3 Qc = (at some temperature) A reaction mixture contains [NO2] = 0.0242 M and [N204] Submit Request Answer 0.0350 M You may want to reference (Pages 653 - 656) Section 15.7 while completing this problem. Part B Determine the direction in which the reaction will proceed. O The reaction proceeds to the right. O The reaction proceeds to the left.
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- PLEASE GO THROUGH AND HELP ME. -the concentration of standard sodium thiosulphate solution is 0.01152 M. -the temperature of the equilibrium mixture in degree Celsius is 20oC. In Determination #1: Volume of thiosulphate = 32.50 mL Volume of Aqueous aliquot = 10.15 mL Strength of Thiosulphate = 0.01152 M In Determination #2: Volume of thiosulphate = 32.50 mL Volume of Aqueous aliquot = 10.23 mL Strength of Thiosulphate = 0.01152 M In Determination #3: Volume of thiosulphate = 32.67 mL Volume of Aqueous aliquot = 10.31 mL Strength of Thiosulphate = 0.01152 M https://drive.google.com/file/d/1824fGKn1AMdByzDsSLq8Nv323rpC4e79/view?usp=sharingFor a 22.16 mg sample of MgC2O4•H2O (Mwt = 130.35 g/mol) shows two steps:a loss of 3.06 mg from 100–250 oC and a loss of 12.24 mg from 350–550oC. For each step, identify the volatilization product and the solidresidue that remains. In second step, two volatile products are formed.(Mwt C = 12 g/mol; O = 16 g/mol; H = 1 g/mol)1. Instructor Date Section Station The solubility of magnesium hydroxide (Mg(OH)2) is approximately 3.70 x10−5 M at room temperature. Write the aqueous dissolution ionic reaction for magnesium hydroxide. Include state symbols. Calculate the solubility product constant (Ksp) for magnesium hydroxide at room temperature. Refer back to the General Formula for “K” presented in the “Equilibrium Lab Manual” . 2. 3. c. How many grams of magnesium hydroxide are present in 1.0 L of a saturated solution at room temperature? An Excel plot of ln K vs. �??1� a slope value of −2980 K and an intercept of −10.6. Show all work using Dimensional Analysis to calculate ∆H° in kJ/mol and ∆S° in J⋅K−1⋅mol−1. Hint: Write out the equation for this line in terms of K, T, ∆H° and ∆S° to start with. By setting ∆G = 0 in Eqn. 5, use the Lit values above to solve for “T” below. (Hint: “T” is the only unknown left in that equation now.)
- . A solution was prepared by mixing 4.00mL of 2.00 x 10-3 M Fe(NO3)3 and 3.00mL of 5.00 x 10-3 M NaSCN and diluting the mixture with water to a total of 10.00mL. Use your average value of Kc to calculate the equilibrium concentration of FeSCN2+ in the mixture. [Hint: Use as many significant figures as you legitimately can in your calculations] my average you can find on the picture below PLS HELP ASAP!!Evaluate the starting amounts in the following experiments and determine whether the reaction will proceed in the forward direction, reverse direction, or whether it is at equilibrium. The equilibrium constant for the reaction N2(g) + 3 H2(g) ⇋ 2 NH3(g) is 6.0 x 105 at 298K. Experiment N2 H2 NH3 Proceed forward or reverse? 1 0.02 M 0.01 M 0.8 M forward/reverse/at equilibrium 2 0.8 M 0.2 M 0.8 M forward/reverse/at equilibrium 3 0.2 M 0.2 M 0 MUse the Le Châtelier's Principal with a conversion rate of 30% A→B and 45% B→A. After reaching equilibrium, adjust the quantities to A=10 and B=90. How many additional time iterations (rows) are required before equilibrium is re-established (i.e. when the number you type on the left first equals the number you type on the right)?
- At equilibrium, the concentrations in this system were found to be [N₂] = [O₂] = 0.200 M and [NO] = 0.500 M. N₂(g) + O₂(g) = 2NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-established? [NO] final = M Note:- • Do not provide handwritten solution. Maintain accuracy and quality in your answer. Take care of plagiarism. • Answer completely. • You will get up vote for sure.Find calculated k value per trial: Average k value: The initial volume of syringe was 15ml and I converted everything to L because that is what my manual said to do. I am confused with my excel spreadsheet as well. Am I doing my calculations correctly?In the gas phase reaction 2 A(g) + B(g) = 3 C (g) + 2 D (g) it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate (a) the mole fractions of each species, (b) KX, (c) KP and (d) △Go . Answer: [0.087 (A); 0.370 (B); 0.196 (C); 0.348 (D); 0.326; 0.325; 2.76 kJ]
- Given that the following reversible reaction: 2NH3(g) ⇌ N2(g) +3H2(g) ; If 0.64 mols of NH3 is added to an empty 750 mL container and allowed to reach equilibrium at which point the concentration of NH3 = 0.15M, predict the equilibrium concentrations of N2 (g) and H2 (g) answer should follow the format: a) Initial Molarity of (i) NH3(g) (ii) N2(g) (iii) H2(g) b) Change (using + or - x values) (i) NH3(g) (ii) N2(g) (iii) H2(g) c) the value of X d) Equilibrium Molarity of (i) NH3(g) (ii) N2(g) (iii) H2(g)CH4 + 2H2O = CO2+3H2 For the following gas phase reaction,A. Find the equilibrium constant at T= 300°C using the shortcut van‘t Hoff approachA reaction mixture is made of initial: [PCl5] = 0.210 M, [PCl3] = 0.0900 M, [Cl2] = 0.0900M In which direction will the reaction proceed to reach eqºm? Q = ------ = _____Mx______M/_______M > ? < K = 0.042M shifts? If [PCl5]eq = 0.2065 M, find all [conc]eq in this reaction mixture. Set up an ICE table: [PCl5] [PCl3] [Cl2] Init Change Eqºm [PCl5]eq = 0.2065 M = _______ x = _______ M [PCl3]eq = ___________ = _______ M [Cl2]eq = _______ M