The reaction C2H4(g) + N2O(g) --------> CH3CHO(g) +NO(g) is first order in both C2H4 and N2O, with...
The reaction
C2H4(g) + N2O(g) --------> CH3CHO(g) +NO(g)
is first order in both
C2H4 and
N2O, with k =
1.46×10-3 L
(mol^-1)(s^-1) at 580°C. If 1.00 L of
C2H4(g) at a concentration
of 3.50×10-3 M is rapidly mixed with
the same volume of N2O(g) also at a
concentration of 3.50×10-3 M, what is
the time (in seconds) required for the
C2H4 concentration to
decrease to a value of 1.06×10-3
M?
Homework Answers
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The reaction
C2H4(g) +
N2O(g)
--------> CH3CHO(g)
+NO(g)
is first order in both
C2H4 and
N2O, with...
The reaction I2(g) +SiH4(g) -------> HI(g) +SiH3I(g) is first order in both I2 and SiH4, with...
The reaction I2(g) +SiH4(g) -------> HI(g) +SiH3I(g) is first order in both I2 and SiH4, with k = 2.14 L mol-1 s-1 at 255°C. If 1.00 L of I2(g) at a concentration of 2.44×10-3 M is rapidly mixed with the same volume of SiH4(g) also at a concentration of 2.44×10-3 M, what is the time (in seconds) required for the I2 concentration to decrease to a value of 3.38×10-4 M? HINT: Because the reaction conditions and stoichiometry are such that...
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1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order in H2O2 and has a rate constant k = 1.06×10−3 min−1 at a given temperature. How long will it take for 15% of a sample of H2O2 to decompose? 2)The decomposition of nitrogen dioxide, NO2, into nitrogen monoxide and oxygen at a high temperature is second-order in NO2. The rate constant for this reaction is 3.40 L/mol×min. Determine the time needed for the concentration...
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Consider the following reaction: 2 N2O(g) → 2 N2(g)+O2(g) A) Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. ans: Rate= −1/2 Δ[N2O] / Δt= 1/2 Δ[N2] / Δt = Δ[O2] / Δt B) In the first 13.0 s of the reaction, 1.7×10−2 mol of O2 is produced in a reaction vessel with a volume of 0.440 L . What is the average rate of the reaction over this time interval? ans:...
The decomposition of nitramide in aqueous solution at 25°C NH2NO2(aq) N2O(g) + H2O(1) is first order...
The decomposition of nitramide in aqueous solution at 25°C NH2NO2(aq) N2O(g) + H2O(1) is first order in NH NO2 with a rate constant of 4.70x10-55-1 If the initial concentration of NH_NO2 is 0.902 M, the concentration of NH2NO2 will be M after 45290s have passed In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N205(8) +2 NO2(g) + O2(g) the concentration of N2O5 was followed as a function of time It was found that a...
Consider the following reaction: 2 N2O(g) → 2 N2(g)+O2(g) Part A: In the first 15.0 s...
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2. The activation energy for the following first-order reaction is 102 kJ/mol. N2O(g) → 2NO(g) +...
2. The activation energy for the following first-order reaction is 102 kJ/mol. N2O(g) → 2NO(g) + 1/2O2(g) The value of the rate constant (k) is 1.35 x 10-s-1 at 35°C. What is the value of k at 20°C? (6 points)
Consider the following reaction: 2 N2O(g) → 2 N2(g)+O2(g). In the first 10.0 s of the...
Consider the following reaction: 2 N2O(g) → 2 N2(g)+O2(g). In the first 10.0 s of the reaction, 1.9×10−2 mol of O2 is produced in a reaction vessel with a volume of 0.280L. What is the average rate of the reaction over this time interval? Predict the rate of change in the concentration of N2ON2O over this time interval. In other words, what is Δ[N2O]Δ over Δ[N2O]Δt?
The decomposition of nitramide in aqueous solution at 25°C NH2NO2(aq) N2O(g) + H2O(1) is first order in NH NO2 with a rate constant of 4.70x10-55-1 If the initial concentration of NH_NO2 is 0.902 M, the concentration of NH2NO2 will be M after 45290s have passed In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N205(8) +2 NO2(g) + O2(g) the concentration of N2O5 was followed as a function of time It was found that a...
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