At a certain temperature, initial rate data for the decomposition of gaseous N2O5 are as follows:
Experiment Initial [N2O5] Initial Rate of Decomposition of N2O5
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a) What is the rate law
b) What is the value of the rate constant, including the proper units?
c) What is the initial rate of decomposition of N2O5 when its initial concentration is 0.030M?
At a certain temperature, initial rate data for the decomposition of gaseous N2O5 are as follows:...
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 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
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...
10. Initial rate data have been determined at a certain temperature for the gaseous reaction: 2NO + 2 H2 → N2 + 2 H20 [NO], [Hz]. Initial Rate (M/s) 0.10 0.20 0.0150 0.10 0.30 0.0225 0.20 0.20 0.0600 The numerical value of the rate constant is: (what are the units?) a. 380 b. 0.75 c. 7.5 d. 3.0 x 10-3
Consider this initial-rate data at a certain temperature for the reaction described by 2NO2(g)+O3(g) ----> N2O5(g) + O2(g) [NO2]0 (M) [O3]0(M) Initial rate (M/s) 0.650 0.800 2.47x10^4 1.10 0.800 4.18x10^4 1.76 1.40 11.70x10^4 Determine the value and units of the rate constant. K=_____
The rate constant for the first-order decomposition of N2O5 is 2.81×10−2 s−1 at 20∘C. If the initial concentration of N2O5 is 2.50 M, what is the [N2O5] after 100 seconds?
The decomposition of N2O5 in the gas phase was studied at constant temperature. 2 N 2O5(g) → 4 NO2(g) + O2(g) The following results were collected: [N 2O5] Time (s) 0.1000 0 0.0707 50 0.0500 100 0.0250 200 0.0125 300 0.00625 400 (a) Determine the rate law and calculate the value of k. (b) Determine the concentration of N2O5(g) at 250 s. Does your calculated answer make sense? Justify your answer. (c) Determine the concentration of N2O5(g) at 600...
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...
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 rate constant for the decomposition of N,Os(8) at a certain temperature is 1.70x10sl. (a) If the initial concentration of N;O(8) is 0.200 mol/L, How long will it take for the concentration to fall to 0.100 mol/L? (b) What will the concentration of N:Os(8) be after 16 hours of reaction?