For a first order reaction k = 1/t ln [a0/a]
a0 = 0.36M
a = 0.30M
t = 15 min
hence k = 1/15 ln [0.36/0.30] = 0.012 min-1
Ethyl iodide (C2H5I) decomposes at a certain temperature in the gas phase as follows C2H5I(g) rightarrow...
10) Ethyl iodide (C2H5I) decomposes at a certain temperature in the gas phase as follows: C2H5I(g) → C2H4(g) + HI(g) From the following data determine the order of the reaction and the rate constant. Time (min) [C2H5I] (M) 0.0 2.00 15.0 1.82 30.0 1.64 48.0 1.42 75.0 1.10 1) Reaction order: a) 0 b) 1 c) 2 2) Rate Constant: (enter only the numerical value of the rate constant). _______
Jump Be sure to answer all parts. Ethyl iodide (C_H31) decomposes at a certain temperature in the gas phase as follows: CHşl()+CH () + HI(g) From the following data determine the order of the reaction and the rate constant. Time (min) [CHI] (M) 0. 0 2 .00 0 1.85 1.70 11.52 11.25 Reaction order: 0 1 Rate Constant: (enter only the numerical value of the rate constant). < Prev
Be sule to answer all parts Ethyl iodide (C2Hgl) decomposes at a certain temperature in the gas phase according to first-order kinetics as follows: The rate constant for this reaction is k-228x 10-*s-1. Use it to fill in the missing values in the following table: Time (min) [C2H;I (M) 0.49 10 20 30 40 [C2Hsll1o min -0.392 [C2H51]20 min-10.365 I 2115130 min IC2Hs1l40 min 0.277
1/ The Following data was obtained while observing a reaction between nitric oxide and hydrogen: F2(g) + 2CLO2(g) -----> 2FCLO2(g) Experiment Initial(F2) Initial(CLO2) Initial rate (mol/L) (mol/L) (mol/L*s) 1/ 0.10 0.010 1.2 x 10^-3 2/ 0.10 0.040 4.8 x 10^-3 3/ 0.20 0.010 2.4 x 10^-3 A/ write the rate law for this reaction B/ calculate the rate constant for the reaction C/ what is the order of this reaction 2/ consider the reaction N2(g) + 3H2(g) ----> 2NH3(g). At...
In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)½ H2(g) + ½ I2(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.68×10-3 M-1 s-1 and a y-intercept of 2.66 M-1. Based on this plot, the reaction is ______ (zero/first/second) order in HI and the rate constant for the reaction is _____...
Hydrogen iodide gas decomposes into hydrogen gas and iodine gas at 453°C. If a 2.00 L flask is filled with 0.200 mol of hydrogen iodide gas, 0.156 mol hydrogen iodide remains at equilibrium. What is the equilibrium constant, Kc. for the reaction at this temperature? 2 HI (g) ⇌ H2 (g)+ I2 (8) 0.020 0.0062
The gas phase decomposition of hydrogen iodide at 700 K HI(g) H,(g) + % 13(8) is second order in HI In one experiment, when the initial concentration of HI was 2.42 M, the concentration of HI dropped to 0.348 M after 1.48X10 seconds had passed. Based on these data, the rate constant for the reaction is M's
The gas phase decomposition of hydrogen iodide at 700 K
HI(g)½
H2(g) + ½ I2(g)
is second order in HI with a
rate constant of 1.20×10-3
M-1 s-1.
If the initial concentration of HI is
2.22 M, the concentration of HI
will be _____________________M after
2.21×103 seconds have
passed.
The gas phase decomposition of hydrogen iodide at 700 K HI(g)%H2(g) + 12() is second order in HI with a rate constant of 1.20x10-'M',' If the initial concentration of HI is 1.48 M, the concentration of HI will be M after 1.34x10 seconds have passed.
1a. Hydrogen iodide decomposes when heated, forming H2 (g) and I2 (g). The rate law for this reaction is -delta[HI]/delta t = k[HI]^2. At 443 °C, k=30.L/molxmin. If the initial HI (g) concentration is 5.5x10^-2 mol/L, what concentration of HI (g) will remain after 10. minutes? Concentration = ____ mol/L 1b. The decomposition of SO2Cl2 SO2Cl2 (g) ----> SO2 (g) + Cl2 (g) is first-order in SO2Cl2, and the reaction has a half-life of 245 minutes at 600 K. If...