Write the rate law for the following reactions:
a. 2N2O5 (g) = 4NO2 (g) +2 (g)
b. H2 (g) + I2 (g) = 2HI (g)
c. O2 (g) + O (g) = O3 (g)
Write the rate law for the following reactions: a. 2N2O5 (g) = 4NO2 (g) +2 (g)...
Part A There are six different reactions you can access in the simulation using the drop-down menu. Which of the following are second-order reactions? Check all that apply. Check all that apply. C2H6→2CH3 2N2O5→4NO2+O2 2N2O→2N2+O2 2HI→H2+I2 2NO2→2NO+O2
The decomposition of N2O5 is described by the following equation. 2N2O5(g) → 4NO2(g) + O2(g) If the rate constant is 2.50 × 10−4 s−1, what is the half-life of this reaction?
The decomposition of N2O5 in carbon tetrachloride proceeds as follows: 2N2O5→4NO2+O2 The rate law is first order in N2O5. At 64*C the rate constant is 4.82 ×10^−3s^−1 The rate law is 4.82x10-3s-1 [N2O5] The rate of rxn when [N2O5]=2.40x10^-2 M is 1.16x10^-4 M/s What happens to the rate when the concentration of N2O5 is doubled? What about halved? The answers are NOT 9.64x10^-3 and 2.41x10^-3 M/s
8. Which of the following reactions cannot proceed through a single elementary step in view of the experimental rate law given? (a) NO(g) + O3(g) ⟶ NO2(g) + O2(g) rate = k[NO][O3] (b) 2HI(g) ⟶ H2(g) + I2(g) rate = k[HI]2 (c) C4H8(g) ⟶ 2C2H4(g) rate = k[C4H8] (d) 2NO(g) + H2(g) ⟶ N2(g) + H2O(g) rate = k[NO][H2] (e) 2NO(g) + Cl2(g) ⟶ 2NOCl(g) rate = k[NO]2[Cl2] The worksheet says that the answer is D, but I don’t get...
1A. Consider the following combustion reaction: 2N2O5 (g) à 4NO2(g) + O2(g) For this reaction, show how the rate formation of nitrogen dioxide is related to rate of reaction of nitrogen pentoxide. What would it be for Oxygen to nitrogen dioxide? 1B. Given: Rate = k [A] [B]2 [C]2 What is the order of the reaction with respect to each letter? What is the overall order of the reaction?
6) The rate constant for the first-order decomposition of N2O5 in the reaction 2N2O5(g) → 4NO2(g) + O2(g) is k=3.38 x 10-5 s-1 at 25°C. What is the half-life of N2O5? What will be the total pressure, initially 88.3 kPa for the pure N2O5 vapour, (a) 10 s, (b) 10 minutes after initiation of the reaction?
The decomposition of dinitrogen pentoxide is described by the chemical equation 2N2O5(g) → 4NO2(g) + O2(g). If the rate of appearance of O2 is equal to 2.60 mol min-1 at a particular moment, what is the rate of disappearance of N2O5 at that moment?
Consider the reaction 4NO2(g)+ O2(g)→ 2N2O5(g) At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of 0.0014 M/s. What rate is the molecular oxygen being consumed?
20. Consider the reaction 2N2O5(g)4NO2(g) + O2(g) at 25 C for which the following data are relevant: Дн 13.30 kJ/mol 355.7 J/K mol N205 33.15 kJ/mol 239.9 J/K mol NO2 0 kJ/mol 204.8 J/K mol О2 Calculate AG° for the reaction at 25°C a. 1.35 x 105 kJ b. 94.7 kJ c. -29.0 kJ d. 135 kJ е. O kJ
The first-order rate constant for the decomposition of N2O5, 2N2O5(g)→4NO2(g)+O2(g) at 70∘C is 6.82×10−3 s−1. Suppose we start with 2.40×10−2 mol of N2O5(g) in a volume of 2.1 L. a) How many moles of N2O5 will remain after 7.0 min? b) How many minutes will it take for the quantity of N2O5 to drop to 1.6×10−2 mol?