A.) The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g) 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.363 moles of H2 and 0.363 moles of I2 are introduced into a 1.00 L vessel at 698 K.
A.) The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g) 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.363 moles of H2 and 0.363 moles of I2 are introduced into a 1.00 L vessel at 698 K.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 38GQ: At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g)...
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A.) The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K.
H2 (g) + I2 (g) 2 HI (g)
Calculate the equilibrium concentrations of reactants and product when 0.363 moles of H2 and 0.363 moles of I2 are introduced into a 1.00 L vessel at 698 K.
H2 (g) + I2 (g) 2 HI (g)
Calculate the equilibrium concentrations of reactants and product when 0.363 moles of H2 and 0.363 moles of I2 are introduced into a 1.00 L vessel at 698 K.
| [ H2 ] | = | M |
| [ I2 ] | = | M |
| [ HI ] | = | M |
B.) The equilibrium constant, Kc, for the following reaction is 7.00×10-5 at 673 K .NH4I(s) NH3(g) + HI(g) Calculate the equilibrium concentration of HI when 0.234 moles of NH4I(s) are introduced into a 1.00 L vessel at 673 K.
[HI] = M
[HI] = M
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