2HI (g) H2(g) + I2(g)The rate equation for the reaction is rate = k[HI]²At 629 K and at a concentration of 2.00 mol dm-3, the rate of decomposition of hydrogen iodide = 24.0 x 10-5mol dm-3s-2. a)Calculate the rate constant, k, for the reaction at 629K. Give the units .b)Calculate the number of hydrogen iodide molecules that decompose per second in 1 dm³of gaseous hydrogen iodide at 629K (at concentration 2.00 mol dm-3).
2HI (g) H2(g) + I2(g)The rate equation for the reaction is rate = k[HI]²At 629 K and at a concentration of 2.00 mol dm-3, the rate of decomposition of hydrogen iodide = 24.0 x 10-5mol dm-3s-2. a)Calculate the rate constant, k, for the reaction at 629K. Give the units .b)Calculate the number of hydrogen iodide molecules that decompose per second in 1 dm³of gaseous hydrogen iodide at 629K (at concentration 2.00 mol dm-3).
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 116QRT
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2HI (g) H2(g) + I2(g)The rate equation for the reaction is rate = k[HI]²At 629 K and at a concentration of 2.00 mol dm-3, the rate of decomposition of hydrogen iodide = 24.0 x 10-5mol dm-3s-2.
a)Calculate the rate constant, k, for the reaction at 629K. Give the units
.b)Calculate the number of hydrogen iodide molecules that decompose per second in 1 dm³of gaseous hydrogen iodide at 629K (at concentration 2.00 mol dm-3).
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