HI dissociates to form I2 and H2: If the concentration of HI changes at a rate...
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Determine As for the reaction Zn(s) + 2 HCl(aq) Substance Zn(s) HCl(aq) H2(8) ZnCl2(aq) ZnCl(aq) + H2(g) given the following information: Sº (J/mol x K) 41.6 56.5 130.6 0.9 -33.4 J/K 0-23.1 J/K +23.1 J/K Оозик +33 4 J/K HI dissociates to form 12 and H2:2 HI(g) → H,()+1() If the concentration of HI changes at a rate of -0.45 M/s, what is the rate of appearance of 12(g)? 0.90 M/S 0.13 M/s 1.0 m/s 0.45...
The reaction 2HI → H2 + I2 is second order in [HI] and second order overall. The rate constant of the reaction at 700°C is 1.57 × 10−5 M −1s−1. Suppose you have a sample in which the concentration of HI is 0.75 M. What was the concentration of HI 8 hours earlier? A) 0.45 M B) 0.75 M C) 2.3 M D) 1.9 M
Consider the second-order reaction: 2HI(g)→H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. What will be the concentration of HI after t = 5.92×1010 s ([HI]t) for a reaction starting under the condition in the simulation?
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 following reaction: H2 (g) + I2 (g) ⇋ 2 HI (g) Has an equilibrium constant of 30.5 under certain conditions. If initial concentrations of reactants and product are: [H2] = 0.100 M; [I2] = 0.100 M; and [HI] = 0.250 M, what will be the equilibrium concentration of HI?
The rate constant for the gaseous reaction H2(g) + I2(g) → 2HI(g) is 2.42 × 10−2/(M·s) at 400°C. Initially an equimolar sample of H2 and I2 is placed in a vessel at 400°C and the total pressure is 1690 mmHg. (a) What is the initial rate (M·min) of formation of HI? (__________) (b) What are the rate of formation of HI and the concentration of HI (in molarity) after 13.4 min? Rate of formation = (_______) (c) [HI] = (_______)...
1/2 H2 (g) + 1/2 I2 (g) <-> HI (g) At a certain temperature, Kc of reaction is 400 If 0.025M of H2 and 0.025 M and 0.065 M of HI are in a 1.00 L container, what is the concentration of HI at equilibrium?
Given the equilibrium reaction: 2HI(g) H2(g) + I2(g) A sample mixture of HI, H2, and 12, at equilibrium, was found to have [H2]- 1.4 x 102 Mand [HI 4.0 x 102 M. If Keq 1.0 x 10, calculate the molar concentration of I2 in the equilibrium mixture, Enter your answer in the provided box. ]= м
Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s-1. (a) What is the half-life for this reaction? _______ s (b) If you start with 0.051 M I2 at this temperature, how much will remain after 5.30 s assuming that the iodine atoms do not recombine to form I2? _______ M
consider the equilibrium reaction of H2 (g) + I2 (g) <-----> 2 HI (g) it has an equilibrium constant Kc = 54.3 at 430°C. if the initial concentration of [HI]0 = 2.000 M. what are the equilibrium concentrations?