7. Express the rate of the reaction below in terms of the formation of dinitrogen pentaoxide....
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?
Calculate the Delta H formation of N2O5 (g) given the below reactions: 2NO (g) + O2 (g) -> 2NO2 (g), ΔHrxn = -114.1 kJ/mol 4NO2(g) + O2 (g) -> 2N2O5 (g), ΔHrxn = -110.2 kJ/mol N2 (g) + O2 (g) -> 2 NO (g), ΔHrxn = +180.5 kJ/mol
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?
Write a balanced reaction for which the following rate relationships are true: Rate = -1/2 delta[N2O5] over delta t = 1/4 delta[NO2] over delta t = delta]O2] over delta t a. 2N2O5 yields 4NO2 + O2 b. 4NO2 + O2 yields 2N2O5 c. 2N2O5 yields NO2 + 4O2 d. 1/4 NO2 + O2 yields 1/2 N2)5 e. 1/2 N2O5 yields 1/4 NO2 + O2 Can someone please describe WHY the answer is A? Please show work.
Dinitrogen pentaoxide rapidly decomposes in the atmosphere according to the reaction 2 N2O5(g)-->2 N2O4(g)+ O2(g). At a particular temperature, the slope of a plot of ln[N2O5] versus time is -0.00693. How long will it take N2O5 to reach 0.100% of its original concentration if [N2O5]0= 0.0250M?
Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp for the reaction at 298 K. A. 7.63 x 10-7 B 660 C. 54 D. 2.74 x 104 10 E Consider the following reaction: 2N2O5(g) 4NO2(g) + O2(g) If AH°xn = 110 kJ mol-1 and AS°,n = 454 J-K-1-mol-1 at 298 K, calculate the value of the equilibrium constant Kp...
Need answer and explanation I. For the reaction 2 A+3B → 4C+5D, the rate ofthe reaction in terms ofAA would be written as 2.For the reaction 2A 4B + 3D, the rate of the reaction in terms of AB would be written as 3.For the reaction 2A+3B4C+5D, the rate of the reaction in terms of AD would be written as a. +AD/A c. +15 ADA One reaction that occurs in an automobile catalytic converter is the conversion of nitrogen monoxide...
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?
7) The rate constant for the reaction 2N2O5(g) 25°C 4NO2(g) +O2(g) is k = 3.38x10-5/s at a) Enter the half-life of N20s in seconds. Use two significant figures and do not enter units b) Enter the total pressure in kPa 10 seconds after initiation of the reaction if initially there was 88.3kPa of pure N2O5 vapor. Use two significant figures and do not enter the units c) Enter the total pressure in kPa 10 minutes after initiation 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?