At 427 oC the decomposition of hydrogen iodide is second order, according to the following equation: 2Hl -> H2 +I2
In an experiment the initial [Hl]0 = 2.20 M and the rate constant is 0.00142 M-1 s-1.
a) What is the half life in seconds?
b) How much Hl remains after 3600 seconds have passed?
c) How many minutes would it take for a concentration of 1.35 M Hl to decompose to 0.8253 M?
(a) half life = 320. seconds
(b) amount of HI remaining = 0.180 M
(c) time = 5.53 minutes
At 427 oC the decomposition of hydrogen iodide is second order, according to the following equation:...
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)½ H2(g) + ½ I2(g) is zero order in HI. In one experiment, when the initial concentration of HI was 0.433 M, the concentration of HI dropped to 0.100 M after 1.74×10^3 seconds had passed. Based on these data, the rate constant for the reaction is M s-1.
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.
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)½ H2(g) + ½ I2(g) is zero order in HI with a rate constant of 1.20×10-4 M s-1. If the initial concentration of HI is 0.474 M, the concentration of HI will be_________ M after 3.52×103 seconds have passed.
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.
At 36°C, the decomposition of hydrogen iodide into hydrogen and iodine is a second-order reaction. The rate constant for the reaction at 36°C is 0.080 L*mol-1*5-1. How long does it take an initial concentration of 0.120 mol/L to reduce to one-fifth the initial concentration? Enter your answer as a time in seconds with one decimal place. A: 177.1 B: 235.6 C: 313.3 D: 416.7 E: 554.2 F: 737.0 G: 980.3 H: 1303.8 Submit Answer Tries 0/3
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
Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order in HI and the rate constant is 9.7×10−6M−1s−1. Part A What is the half-life (in days) of this reaction when the initial HI concentration is 0.120 M ? Express your answer using two significant figures. t1/2 t 1 / 2 = days Previous AnswersRequest Answer Incorrect; Try Again; 4 attempts remaining Part B How many days does it take for the concentration of HI...
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...
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 _____...
The decomposition reaction of A to B is a first-order reaction with a half-life of 6.19×102 seconds: A → 2B If the initial concentration of A is 0.147 M, how many minutes will it take for the concentration of A to be 18.5% of the initial concentration?