)A nickel catalyst is commonly used in the hydrogenation of ethylene. If the initial concentration of ethylene is 2.75 mol·L−1 and the rate constant for the reaction is 0.0018 mol·L−1·s−1, what is the rate of reaction if it follows a zero-order reaction mechanism? Express your answer to two significant figures. b)Determine the half-life for the reaction in Part B. Express your answer to two significant figures.

Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0094 M·s: 2 NH3 (g) → N2 (g)+3 H, (g) Suppose a 450. mL flask is charged under these conditions with 400. mmol Of ammonia. After how much time is there only 200. 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.

The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C∘C is 6.82×10^−3 s−1. Suppose we start with 2.60×10−2 mol of N2O5(g) in a volume of 1.7 L. How many minutes will it take for the quantity of N2O5 to drop to 1.7×10−2 mol?

Half-life equation for first-order reactions: t1/2=0.673k  where t1/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s−1). A certain first-order reaction has a rate constant of 6.50×10−3 s−1. How long will it take for the reactant concentration to drop to 16 of its initial value? Express your answer with the appropriate units.

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

Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of ·0.0011Ms−1:2NH3(g)→N2(g)+3H2(g)    Suppose a 5.0L ⁢ flask is charged under these conditions with  450.mmol of ammonia. After how much time is there only  225.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.

One of the reactions that occurs in polluted air in urban areas is 2NO2(g) + O3(g) –→N2O5(g) + O2(g). Assume that a species with the formula NO3 is involved in the mechanism, and the observed rate law for the overall reaction is rate = k[NO2][O3]. Propose a mechanism for this reaction that includes the species NO3 and is consistent with the observed rate law. NO2(g) + O3(g) – NO3(g) + O2(g) (fast) NO3(g) + NO2(g) → N2O5(g) (slow) NO2(g) + O3(g) – NO3(g) + O2(g) (fast) 4NO3(g) 2N2O5(g) + O2(g) (slow) NO2(g) + O3(g) –→ NO3(g) + O2(g) (slow) NO3(g) + NO2(g) → N2O5(g) (fast) NO2(3) + O3(g) → NO3(g) + O2(g) (slow) 4NO3(3) → 2N20O5(g) + O2(g) (fast)

The decomposition of NOBr is studied manometrically because the number of moles of gas changes; it cannot be studied colorimetrically because both NOBr and Br2 are reddish-brown. 2NOBr(g)→2NO(g) + Br2(g) Use the data below to make the following determinations: (a) the average rate of decomposition of NOBr over the entire experiment. (b) the average rate of decomposition of NOBr between 2.00 and 4.00 seconds.  Time (s)   [NOBr] (mol/L)   0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033 The rates of decomposition of NOBr are: (a) _______ mol L−1 s−1 (b) _______ mol L−1 s−1

In the presence  of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is 1.27/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 decijal positions.

The reaction A + 2 B → C has the rate law rate = k[A][B]. By what factor does the rate of reaction increase when both [A] and [B] are doubled? What is the half-life for a particular reaction if the rate law is rate = (1301 min⁻¹)[A]? Identify the molecularity of the elementary reaction below: 2NO(g) + Br₂(g) → 2NOBr(g) The following reaction is at equilibrium in a closed 4L vessel: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) What will happen if the vessel volume is reduced to 3L? (Assume constant temperature.) If Kc = 82 for the reaction below at 200 K, then what is the value of Kp? 2 NO₂ (g) ⇌ N₂O₄ (g) Consider the reaction: N₂ (g) + 3 Br₂ (g) ⇌ 2 NBr₃ (g) At equilibrium, the concentrations of N₂ and Br₂ are 0.34 M and 0.70 M respectively, and the concentration of NBr₃ is 0.090 M. What is Kc for this equilibrium?