In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is 1.87/s. Fe3+(aq) + SCN-(aq)  → Fe(SCN)2+(aq). How many seconds would be required for the initial concentration of Fe3+ to decrease to 12.5% of its initial value?  Express your answer to two decimal positions.

Consider the hypothetical reaction A +B+ 2C → 2D + 3E where the rate law is ΔΙΑ = k[A][B]? At Rate An experiment is carried out where [A]o = 1.0 x 10-² M, [B]o 6.0 M, 2 and [C, = 2.0 M. The reaction is started, and after 5.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. -2 k = L² mol -1 S b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 19.0 seconds. Concentration M d. Calculate the concentration of C after 19 seconds. Concentration = M

The gas phase decomposition of nitrosyl chloride at 400 K NOCI(g)- →NO(g) + ½ Cl2(g) is second order in NOCI with a rate constant of 5.90x10-4 M-1 s1. If the initial concentration of NOCI is 7.40x10-2 M, the concentration of NOCI will be 1.65x10-2 M after seconds have passed.

In the presence  of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is (1.47x10^0)/s. Fe3+(aq) + SCN-(aq)  → Fe(SCN)2+(aq). What is the half-life, in seconds, of the reaction? Express your answer to three significant figures.

Under certain conditions the rate of this reaction is zero order in hydrogen lodide with a rate constant of 0.0038 M's ': 2 HI(g) H,(g)+1,(g) Suppose a 4.0L flask is charged under these conditions with 100, mmol of hydrogen lodide. After how much time is there only 50.0 mmol left? You may assume no other reaction Is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.

The first-order rate constant for the decomposition of N2O5, 2N2O5(g) yields 4NO2(g) at 70∘C is 6.82 x 10-3 s-1 . Suppose we start with 2.30×10−2 mol of N2O5(g) in a volume of 1.8 L .  How many moles of N2O5 will remain after 7.0 minutes?

The initial concentration of NOCl in the second-order reaction 2NOCl→2NO+Cl2 is 0.878M. After 763,200 seconds, the concentration of NOCl is 0.83M. What is the rate constant k for the reaction?

In the presence of excess thiocyanate ion, , the following reaction is first order in iron(III) ion, . The rate constant is 1.27/s. Fe3+(aq) + SCN- (aq) --> Fe(SCN)2+ (aq) If 89.9% of the reaction is required to obtain a noticeable color from the formation of the ion, Fe(SCN)2+ ion, how many seconds are required?

7.) The results of kinetics experiments have shown the rate of the following reaction:A + 2B + C ↓ products has the following rate law: rate = k[A]2[B]0[C]1with a rate constant of k = 1.3 × 10–4 L2/mole2·s (M –2·s–1).a.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 0.3, and 0.4 M, respectively?b.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 2.7, and 0.4 M, respectively?

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0094 M-s 2 HI (g) → H, (g) +1, (8) Suppose a 2.0 L flask is charged under these conditions with 100. mmol of hydrogen iodide. After how much time is there only 50.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. Submit Assignm Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center | Accessil 43,203 18 MacBook Air F10 F9 F7 吕口 F3 O00 F4 F5 olo