Hydrogen iodide decomposes when heated, forming H2(g) and I2(g). The rate law for this reaction is âÎ[HI]/ Î t = k[HI]2. At 443 Â°C, k = 30. L/molÂ·min. If the initial HI(g) concentration is 4.7 x 10^-2 mol/L, what concentration of HI(g) will remain after 8.0 minutes?

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13 Dec 2019

Hydrogen iodide decomposes when heated, forming H₂(g) and I₂(g). The rate law for this reaction is âÎ[HI]/ Î t = k[HI]². At 443 Â°C, k = 30. L/molÂ·min. If the initial HI(g) concentration is 4.7 x 10^-2 mol/L, what concentration of HI(g) will remain after 8.0 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?

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Hydrogen iodide decomposes when heated, forming H₂(g) and I₂(g). The rate law for this reaction is âÎ[HI]/ Î t = k[HI]². At 443 Â°C, k = 30. L/molÂ·min. If the initial HI(g) concentration is 4.7 x 10^-2 mol/L, what concentration of HI(g) will remain after 8.0 minutes?

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Hydrogen iodide decomposes when heated, forming H2(g) and I2(g). The rate law for this reaction is âÎ[HI]/ Î t = k[HI]2. At 443 Â°C, k = 30. L/molÂ·min. If the initial HI(g) concentration is 4.7 x 10^-2 mol/L, what concentration of HI(g) will remain after 8.0 minutes?

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Related textbook solutions

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Hydrogen iodide decomposes when heated, forming H₂(g) and I₂(g). The rate law for this reaction is âÎ[HI]/ Î t = k[HI]². At 443 Â°C, k = 30. L/molÂ·min. If the initial HI(g) concentration is 4.7 x 10^-2 mol/L, what concentration of HI(g) will remain after 8.0 minutes?