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18 Nov 2019

Hydrogen iodide decomposes when heated, forming H2 and I2. The rate law for this reaction is - delta(HI)/delta t= K(HI)^2. At 443 degrees Celsius, K= 30 L/mol min. If the initial HI concentration is 1.5 x 10^-2 mol/L, what concentration of HI will remain after 10 minutes?

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The decomposition of hydrogen iodide on finely divided gold 150C is zero enter with respect to HI. The rate defined below isconstant at 1.20X10-4 mol/L -s

2HI (g) -----> H2 (g) + I2 (g)
Rate = Delta (HI)/ Delta R= k = 1.20 x 10-4 mol/L -s

A.If the initial HI concentration was 0.250 mol/L, calculate theconcentration of HI at 25 minutes after the start of thereaction.

B. How long will it take for all the 0.250 M HI todecompose?

silverhyena89

Any help would be greatly appreciated:

Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order in HI and the rate constant is 9.7Ã10â6Mâ1sâ1. If the initial concentration of HI is 0.120 M:

(A) what is the molarity after 6 days (_______M)

(B) how many days will it take for the reaction to reach a value of 8.5 x 10^-2M (_________days)

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Hydrogen iodide decomposes when heated, forming H2 and I2. The rate law for this reaction is - delta(HI)/delta t= K(HI)^2. At 443 degrees Celsius, K= 30 L/mol min. If the initial HI concentration is 1.5 x 10^-2 mol/L, what concentration of HI will remain after 10 minutes?

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