The rate law for the decomposition of N2O5 is rate = k[N2O5] If k = 1.0...
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 30.0 minutes?
b. What will the CH3CHO concentration be after 180 minutes?
Homework Answers
![1) Rate law: rate *[N2O,] we have k=1.0×10-5 s-1 [Ν,0,1- Thus, 0.0091 mol L-1 rate =小1,0.] = (1.0×10-5 s-1)(0.0091 moll = 9.1](http://img.homeworklib.com/questions/c2ddf440-50cb-11ec-96bb-893ee3fbff77.png?x-oss-process=image/resize,w_560)
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The rate law for the decomposition of N2O5
is
rate = k[N2O5]
If k = 1.0...
the first order decomposition of N2O5 at 328 K has a rate constant of 1.70x10^-3 s^-1....
the first order decomposition of N2O5 at 328 K has a rate constant of 1.70x10^-3 s^-1. if the initial concentration of N2O5 is 2.88 M, what is the concentration of N2O5 after 12.5 minutes?
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). 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
The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3...
The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1. If the initial concentration of N2O5 is 2.88 M, what is the concentration of N2O5 after 12.5 minutes? This is what I did: k = 1.70 x 10^.3 Ao= 2.88M t = 12.5 min Af= ??? I used the equation [Af]= -Kt + ln [Ao] (this equals .0359) which is wrong. What did I do wrong?
the rate law for the decomposition of acetaldehyde is rate=k[ acetaldehyde]^2. what is the rate of...
the rate law for the decomposition of acetaldehyde is rate=k[ acetaldehyde]^2. what is the rate of the reaction when the [acetaldehyde]=1.75x10^-3 M and the rate constant is 6.73x10^-6 M^-1s^-1?
The decomposition of N2O5 in carbon tetrachloride proceeds as follows: 2N2O5→4NO2+O2 The rate law is first...
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
6) The rate constant for the first-order decomposition of N2O5 in the reaction 2N2O5(g) → 4NO2(g)...
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 gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g) 2 NO2(g) + ½ O2(g)...
The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g) 2 NO2(g) + ½ O2(g) is first order in N2O5 with a rate constant of 4.70×10-3 s-1. If the initial concentration of N2O5 is 4.50×10-2 M, the concentration of N2O5 will be ______ M after 259 s have passed.
The reaction 2A + 2B → M + N has the rate law: Rate = k[A]2....
The reaction 2A + 2B → M + N has the rate law: Rate = k[A]2. At 25°C, k = 0.0311 L mol-1 s-1. If the initial concentrations of A and B are 0.321 M and 0.499 M, respectively. What will be the concentrations of A and B after 30.0 minutes?
The first-order rate constant for the decomposition of N2O5, N2O5(g) 2NO2(g) + O2(g)At 70C is 6.810-3s-1....
The first-order rate constant for the decomposition of N2O5, N2O5(g) 2NO2(g) + O2(g)At 70C is 6.810-3s-1. Suppose we start with 0.0250 mol of N2O5(g) in a volume of 1.0 L. a.) How many moles of N2O5will remain after 2.5 min? b.)How many minutes will it take for the quantity of N2O5to drop to 0.010 mol? c.What is the half-life of N2O5at 70 degrees C?
The decomposition of N2O5 in carbon tetrachloride proceeds as follows: What is the rate of reaction...
The decomposition of N2O5 in carbon tetrachloride proceeds as follows: What is the rate of reaction when N205] = 0.0270? Express the rate in molarity per second to three significant figures. 2N2O3 + 4NO2 + O2 The rate law is first order in N2O5. At 64 °C the rate constant is 4.82 x 10-3 3-1 IV AP R O 2 ? You may want to reference (Pages 576 - 581) Section 14.3 while completing this problem. rate = M /S...
The decomposition of N2O5 in carbon tetrachloride proceeds as follows: What is the rate of reaction when N205] = 0.0270? Express the rate in molarity per second to three significant figures. 2N2O3 + 4NO2 + O2 The rate law is first order in N2O5. At 64 °C the rate constant is 4.82 x 10-3 3-1 IV AP R O 2 ? You may want to reference (Pages 576 - 581) Section 14.3 while completing this problem. rate = M /S...
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