The decomposition of N2O5 proceeds according to the following equation 2 N2O5(g) → 4 NO2(g) + O2(g). The rate constant, k, for the reaction at 298 K is 2.20 x 10-3 min-1. If a reaction is set up in a vessel at 298 K, with an initial concentration of 0.278 mol L-1; what is the concentration of reactant N2O5(g) in mol/L after 40.2 minutes? Report your answer without units
Using the rate constant determine the order.
Then determine the integral rate law equation.
Putting the values determine the final concentration.
The decomposition of N2O5 proceeds according to the following equation 2 N2O5(g) → 4 NO2(g) +...
The decomposition of N2O5 proceeds according to the following equation: 2 N2O5 (g) -> 4 NO2 (g) + O2 (g) If the rate of decomposition of N2O5 at a particular instant in a reaction vessel is 5.3 x 10-5 M/s, what is the rate of appearance of NO2?
1A. The decomposition of dinitrogen pentoxide in carbon
tetrachloride solution at 30 °C N2O5 2 NO2 + ½ O2 is first order in
N2O5 with a rate constant of 4.10×10-3 min-1. If the initial
concentration of N2O5 is 0.510 M, the concentration of N2O5 will be
M after 402 min h
1B. The gas phase decomposition of phosphine at 120 °C
PH3(g)1/4
P4(g) + 3/2 H2(g)
is first order in PH3
with a rate constant of 1.80×10-2
s-1.
If the...
3. The rate of decomposition of N2O5 in the reaction 2 N2O5(g) 4 NO2(g) + 5 O2(g) at a particular instant is 4.2 x 10-7 M/s, what is the rate of appearance of NO2?
1a. At 573 K, gaseous NO2 decomposes, forming NO(g) and O2. If a vessel containing NO2(g) has an initial concentration of 0.056 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant, and the rate constant for this reaction, at 573 K, is 1.1 L/mol · s. = ___ s 1b. The decomposition of ammonia on a metal surface to form N2 and H2 is a zero-order reaction....
30) The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N205(g) - 4 NO2(g) + O2(g) If the rate of disappearance of N2O5 is equal to 1.80 mol/min at a particular moment, what is the rate of appearance of NO2 at that moment? 31) The decomposition of dinitrogen pentoxide is described by the following chemical equation 2 N205(g) - 4 NO2(g) + O2(g) If the rate of appearance of NO2 is equal to 0.560 mol/min at...
The decomposition of crystalline N2O5 N2O5 (s) —> 2 NO2 (g) + 1/2 O2 (g) is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25°C we have the following values for the standard state entrapped and free energy changes of the reaction: ΔH° = +109.6 kJ/mol ΔG° = -30.5 kJ/mol a. Calculate ΔS° at 25°C b. Why is the entropy change so favorable for this reaction? Please answer and explain both questions!
The decomposition of NO2 at high temperature NO2(g) → NO(g) + 1/2 O2(g) is a second order process with a rate constant of 3.40 L/mol•min. If an experiment is performed where the initial concentration of NO2 is 0.400 M, what is the concentration of NO2after 2.96 min? [NO2] = M
The rate law for the decomposition of N2O5 is rate = k[N2O5] If k = 1.0 x 10-5 s-1, what is the reaction rate when the N2O5 concentration is 0.0091 mol L-1? 2.The decomposition of acetaldehyde, CH3CHO, was determined to be a second order reaction with a rate constant of 0.0771 M-1 s-1. If the initial concentration of acetaldehyde is 0.301 M , what will the concentration be after selected reaction times? a. What will the CH3CHO concentration be after...
The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction: 2N2O5 (soln) → 4NO2 (soln) + O2 (soln) The reaction is first order and has a rate constant of 4.82 x 10-3 s-1 at 64 oC. The reaction is initiated with 0.058 mol in a 1.25 L vessel. What is the half-life of the reaction?
The decomposition of nitrogen dioxide occurs according to the equation below: NO2 (g)------>NO( g)+1/2 O2 (g) The reaction is second order with respect to NO2. The specific rate constant for this reaction is 3.04M-1min-1. How long does it take for the concentration of NO2 to decrease from 2.00M to 1.25M?