11) The reaction 2NO(g) + 2H₂(g) → N, (g) + 2H₂O(g) was studied at 904°C, and the data in the table were collected. (SHOW CALCULATIONS) Initial Concentrations: Exp. 1 Exp. 2 Exp. 3 [NO] 0.210 M 0.210 M 0.420 M [H₂] 0.150 M 0.300 M 0.150 M Initial Rate 0.0339 M/s 0.0678 M/s 0.136 M/s a) Using the data, determine the order for each reactant. Show any calculations or explain reasoning. b) What is the rate law for the reaction? c) What is the value of the rate constant, k, for this reaction?

Say that you mix Fe3+ and SCN- together so that after mixing, the concentration of Fe3+ (aq) equals 0.0015 M , and the concentration of SCN- (aq) equals 5.5 x 10-4 M. You measure the concentration of product, FeSCN2+, after equilibrium forms. It is 7.2 x 10-5 M. Calculate the value of the equilibrium constant, K, for the reaction.  F e 3 + ( a q ) + S C N − ( a q ) ⟷ F e S C N 2 + ( a q ) K = ? Group of answer choices 0.011 9.52 x 10-3 87.3 105

5. Consider the following reaction: 2A+B C A kinetics study on this reaction yielded the following data: [A] mol/L [B] mol/L Rate = mol/L/s 0.0250 0.0400 4.06 x 10-3 0.0250 0.0800 4.06 x 10-3 0.0500 0.0800 4.06 x 10-3 Calculate the K constant for the above reaction: ()+(p) 28 a a. 0.025 mol/L.s evods A b. 0.0010 mol/L.s c. 0.0020 mol/L.s d. 0.00406 mol/L. s e. None of the above (p) 2 + (p) OS (2):82 svods evil to onait evods all bris ang wond 6. Calculate AG° for the following reaction: Thiog 2 SO2(g) + O2(g) → 2 SO3(g) AGf in kJ/moles for SO2(g) is -300.2, for SO3(g) is -371.1 and for O2 is 0.0. a. +141.8 kJ b. +70.9 kJ c. #70.9 kJ enimmeted d. -141.8 kJ lom EL 7. Consider the following reaction for the production of SO3: 18.8 XC70 b 2 SO2(g) + O2(g) → 2 SO3(g) Which of the following expressions best illustrates the rate of the product? a. rate = 2A[SO3] / At b. rate = A[SO3]/2At c. rate = 2A[SO3]/2At プラ FRASER

Look at the reaction below and state which direction the reaction would shift:   You remove mercury(II) oxide, HgO, from the reaction.   Hint: Remember on the video what I stated about solids!   2HgO (s) <=> 2Hg (l) + O2 (g)

The initial concentration of Cl1- is 0.100M and the initial concentration of Co(H2O)62+ is 0.500 M.  At equilibrium the concentration of CoCl42- is 0.0035.  What is the value of the equilibrium constant for the reaction being studied?

Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.

The elementary reaction 101 4 2H₂O(g) = 2H₂(g) + O₂(g) proceeds at a certain temperature until the partial pressures of H₂O, H₂, and O₂ reach 0.0700 atm, 0.00350 atm, and 0.00300 atm, respectively. What is the value of the equilibrium constant at this temperature? Kp = O R 01 F % 5 1 T a G 6 24 1 & Y H 7 U 8 J 144 ( 9 K BO O O ☐ L Resources DDI P { 2. ✈ ? 59°F [ insert pause prt sc Hint 10/1/2022 backspace delete home enter pg ur T shift in er

How long will it take for the concentration of A to decrease from 0.910 M to 0.573 for the reaction A → Products? (k = 0.153 M/s)