2.1 The reaction of nitrogen dioxide and carbon monoxide in the gas state to form carbon dioxide and nitric oxide is represented by the equation: NO2(g) + CO(g) – cO:(9) + NO(g) The following data were collected for the above reaction Experiment No [NO2] (M) [CO] (M) Initial Rate (M/s) 1 5.0 × 104 1.6 x 10-2 1.7 x 10-7 2 5.0 x 104 3.2 x 10-2 1.7 x 10-7 3 1.5 x 103 3.2 x 10-2 1.5 x 106
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- Sodium chlorate crystals are easy to grow in the shape of cubes by allowing a solution of water and sodium chlorate to evaporate slowly. a. If V is the volume of such a cube with side length x, calculate dV/dx when x = 3 mm and explain its meaning (be specific). b. Show that the rate of change of the volume of a cube with respect to its edge length is equal to half the surface area of the cube.In a study of the gas phase decomposition of sulfuryl chloride at 600 KSO2Cl2(g)SO2(g) + Cl2(g)the concentration of SO2Cl2 was followed as a function of time.It was found that a graph of ln[SO2Cl2] versus time in minutes gave a straight line with a slope of -4.34×10-3 min-1 and a y-intercept of -5.20 .Based on this plot, the reaction is _______zerofirstsecond order in SO2Cl2 and the rate constant for the reaction is min-1.The decomposition of SO2Cl2 SO2Cl2(g) --> SO2(g) + Cl2(g)is order 1 with respect to SO2Cl2 and its half-life (t1/2) is 263 minutes at 300oC. Initially, in a 1.0 L container, the partial pressure of SO2Cl2 is 4.00 kPa.a) What will be the partial pressure of SO2Cl2, SO2 and Cl2 after 263 minutes? Answers:P (SO2Cl2): P(SO2): P(Cl2): b) What is the rate constant, k, of this reaction at 300oC?
- The OH radical reacts with itself in a disproportionation type reaction according to the reaction: OH + OH → H2O + O This rate constant at room temperature is 2.69 x 102 M-1 s-1. If the initial concentration of OH is 2.60 x 10-5 M, what is the first half life for the reaction (in seconds)? (the answer should be entered with 3 significant figures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0)Use the Image to solve these problems. 1. What is the order of this reaction with respect to NO2? 2. Write a rate law for this reaction, and calculate the value of the rate constant (k). (Report in scientific notation to 3 sig figs without units) Rate law: Rate constant (k): 3. Determine the half-life for this reaction. (Report in scientific notation to 3 sig figs without units) 4. Calculate [NO2] at 2.70 x 104 seconds after the start of the reaction. (Report to 3 sig figs without units)Consider the reaction A+2B⇌CA+2B⇌C whose rate at 25 ∘C∘C was measured using three different sets of initial concentrations as listed in the following table: Trial [A][A](MM) [B][B](MM) Rate(M/sM/s) 1 0.20 0.010 4.8×10−4 2 0.20 0.020 9.6×10−4 3 0.40 0.010 1.9×10−3 Calculate the initial rate for the formation of CC at 25 ∘C∘C, if [A]=0.50M[A]=0.50M and [B]=0.075M[B]=0.075M. Express your answer numerically in molar per second using two significant figures.
- A reaction increases its rate four times when temperature increases from 250 K to 300 K. What is the activation energy of the reaction? Round off your answer to 3 significant figures and with correct units:Part B: Integrated rate law expressions for zero- and half-order reactionsDerive integrated rate law expressions for half-, one and a half-, and third-order reactions of the form A products where k is the rate constant. Also, deduce the graphical linear relations, units of rate constant k, and expression for half-life, t1/2 , for all cases. Assume that at t = 0 only A is present with an initial concentration of [A]0. Fill in the table below by following the example given for first-order reaction1.Sucrose (C12H22O11)(C12H22O11), which is commonly known as table sugar, reacts in dilute acid solutions to form two simpler sugars, glucose and fructose, both of which have the formula C6H12O6C6H12O6. At 23 ∘C∘C and in 0.5 M HClM HCl, the following data were obtained for the disappearance of sucrose: Time (min)(min) C12H22O11(M)C12H22O11(M) 0 0.316 39 0.274 80 0.238 140 0.190 210 0.146 What is the rate constant?
- 1. The decomposition of aqueous sucrose to form the isomers glucose and fructose is a common organic reaction, which requires a strong catalyst: C12H22O11(aq) + H2O(l) → 2C6H12O6(aq). The following data were collected during the process: Time (min) [C12H22O11] (mol/L) 0 0.316 39 0.274 80 0.238 140 0.190 210 0.146 (a)If we performed a new trial with an initial concentration of sucrose of 0.400 mol/L, what concentration would remain after 4.0 h has passed? 2. Methyl isomerizes to acetonitrile, CH3NC(g) → CH3CN(g) at 215°C. The following data were collected during the process: Time (sec) [CH3NC] (mol/L) 2000 0.0110 5000 0.0059 8000 0.0031 12000 0.0014 15000 0.0007 2. (a)Assuming the process continues, what concentration of methyl isonitrile would we expect after 5.00 h?A certain reactant is consumed in the course of a chemical reaction such that the reactant that remains in the solution at time t in seconds (sec) is given in the following function where the unit of concentration f(t) is in molarity (M). Function: f(t) = (1.25 x 10^-7)(t-800)^2 + (2.00 x 10^-2) Find the rate of disappearance of the reactant from t = 0 to t=400 secIn a study of the gas phase decomposition of sulfuryl chloride at 600 KSO2Cl2(g)SO2(g) + Cl2(g)the concentration of SO2Cl2 was followed as a function of time.It was found that a graph of ln[SO2Cl2] versus time in minutes gave a straight line with a slope of -4.28×10-3 min-1 and a y-intercept of -6.95 . Based on this plot, the reaction is________. (firest, zero, or second) order in SO2Cl2 and the rate constant for the reaction is min-1.