Question 21Hydrogen iodide can be produced by the reversible reaction of hydrogen gas andiodine gas according to:H2(g) + I2(g) = 2HI(g)Keg for this reaction is 2.25 × 10³ at a temperature of 753°C.Calculate the concentration of HI in an equilibrium mixture if theconcentration of H2 is 0.15 M and the concentration of I2 is 0.25 M.(a)2.4 moles of H2(g) and 1.5 moles of I2(g) were placed in a sealed 2.0 Lvessel maintained at a temperature of 753°C. After 2 hours, the number ofmoles of each gas present were as follows.(b)Moles of H2(g)Moles of I2(g)Moles of HI(g)1.70.81.4Show by calculation whether the forward or reverse reaction must increasefor the system to come to a state of dynamic equilibrium.

Given reaction, H2g+I2g⇔2HIgKeq=2.25×103

Question 21 Hydrogen iodide can be produced by the reversible reaction of hydrogen gas and iodine gas according to: H2(g) + I2(g) = 2HI(g) Keg for this reaction is 2.25 x 103 at a temperature of 753°C. (a) Calculate the concentration of HI in an equilibrium mixture if the concentration of H2 is 0.15 M and the concentration of I2 is 0.25 M. (b) 2.4 moles of H2(g) and 1.5 moles of I2(g) were placed in a sealed 2.0 L vessel maintained at a temperature of 753°C. After 2 hours, the number of moles of each gas present were as follows. Moles of H2(g) Moles of I2(g) Moles of HI(g) 1.7 0.8 1.4 Show by calculation whether the forward or reverse reaction must increase for the system to come to state of dynamic equilibrium.

Question 21 Hydrogen iodide can be produced by the reversible reaction of hydrogen gas and iodine gas according to: H2(g) + I2(g) = 2HI(g) Keg for this reaction is 2.25 x 103 at a temperature of 753°C. (a) Calculate the concentration of HI in an equilibrium mixture if the concentration of H2 is 0.15 M and the concentration of I2 is 0.25 M. (b) 2.4 moles of H2(g) and 1.5 moles of I2(g) were placed in a sealed 2.0 L vessel maintained at a temperature of 753°C. After 2 hours, the number of moles of each gas present were as follows. Moles of H2(g) Moles of I2(g) Moles of HI(g) 1.7 0.8 1.4 Show by calculation whether the forward or reverse reaction must increase for the system to come to state of dynamic equilibrium.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 49QAP: Consider the system SO3(g)SO2(g)+12 O2(g)H=98.9kJ (a) Predict whether the forward or reverse...

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