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- If Δ[Br2]ΔtΔ[Br2]Δ� = 4.7×10−6 M/sM/s , what is the value of Δ[ClO−2]ΔtΔ[ClO2−]Δ� during the same time interval? Express your answer to two significant figures and include the appropriate units. What is the average rate of consumption of Br−Br− during the same time interval? Express your answer to two significant figures and include the appropriate units.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 at t=400 secConsider the following data on the natural decomposition of a new molecule, TfO2, discovered in the sap of the Truffula tree in the land of the Lorax. What is the average rate of decomposition (mol/L•min) over the period of time from time point 1 and time point 2? Report your answer to the thousandths place and do not include units. Timepoint Time (min) concentration of TfO2 (mol/L) 1 0 2.341 2 5 1.417 3 16 0.727 4 27 0.38 5 37 0.08
- A bimolecular chemical reaction is one in which two chemicals react to form another substance. Suppose that one molecule of each of the two chemicals reacts to form two molecules of a new substance. If x represents the number of molecules of the new substance at time t, then the rate of change of x is proportional to the square of the numbers of molecules of the original chemicals available to be converted. That is, if each of the chemicals initially contained A molecules, then dx dt = k(A − x)2 where k is a constant. If 40% of the initial amount A is converted after 1 hour, how long will it be before 50% is converted? (Give an exact answer. Do not round.)Consider the following data for the decomposition of N2O5 at 57 degree celsius: t(min) 0 2.0 4.0 6.0 8.0 [N2O5] (M) 0.160 0.126 0.099 0.078 0.061 a. calculate the average rate at 4.0 min using data for 2.0 min and 6.0 min. b plot the given data on a graph and draw a tangent to the curve to find the rate at 4.0 minIn 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.
- A gas, AB, decomposes and the volume of B2 produced is measured as a function of time. The data obtained are as follows: Time (min): 0, 8.3, 15.4, 19 Volume (L): 0, 4.2, 8.6, 11.5 What is the average rate of production of B2 for the first 19 min? Round your answer to 2 decimal places.What is the average rate from t1= 50 s to t2= 100 s1. 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?
- For the decomposition of ammonia on a tungsten surface at 1100 °C 2 NH3(g)-->N2(g) + 3 H2(g) the average rate of disappearance of NH3 over the time period from t= 0s to t = 1.04×103 s is found to be 3.40×10-6 M/s. What is the average rate of appearance of N2 over the same time period?Determine the average rate of change of BB from ?=0 st=0 s to ?=272 s.t=272 s. A⟶2BA⟶2B Time (s) Concentration of A (M) 0 0.7300.730 136136 0.4450.445 272272 0.1600.160 rateB= __________M/sThe decomposition of H2O2 was studied and the concentration (in moles per liter) as a function of time was determined. a. Create a spreadsheet in Excel with the following columns and values. Calculate values for the natural logarithm of [H2O2] using an appropriate formula. Time H2O2(M) LN [H2O2] 0 0.862 120 0.556 240 0.394 360 0.246 480 0.149 b. Create a graph of [H2O2] versus time. Use the Scatter chart type and use the subtype that connect the points with a line. c. Create a graph of LN(H2O2) versus time. Use the scatter chart type and use the subtype that does not connect the points with a line. Instead, insert a trendline (linear fit) and display the equation of the line on the graph. d. Using the trendline equation, calculate the natural log of concentration (LN[H2O2] corresponding to a time elapsed of 200 seconds. From that value, calculate the molar concentration of H2O2 at 200 seconds