At elevated temperatures, ammonium iodide decomposes according to NH4I(s) ⇌ NH3(g) + HI(g) (a) If Kp = 18 bar2, calculate the total pressure, assuming that only NH4I(s) was present initially. (b) What would be the total pressure at equilibrium if the initial pressure of NH3(g) was 5.0 bar, with NH4I(s) but no HI(g) present? (a) 8.5 bar (b) 9.8 bar
At elevated temperatures, ammonium iodide decomposes according to NH4I(s) ⇌ NH3(g) + HI(g) (a) If Kp = 18 bar2, calculate the total pressure, assuming that only NH4I(s) was present initially. (b) What would be the total pressure at equilibrium if the initial pressure of NH3(g) was 5.0 bar, with NH4I(s) but no HI(g) present? (a) 8.5 bar (b) 9.8 bar
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 112CP: Nitric oxide and bromine at initial partial pressures of 98.4 and 41.3 torr, respectively, were...
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At elevated temperatures, ammonium iodide
decomposes according to
NH4I(s) ⇌ NH3(g) + HI(g)
(a) If Kp = 18 bar2, calculate the total pressure, assuming that only NH4I(s) was present initially.
(b) What would be the total pressure at equilibrium if the initial pressure of NH3(g) was 5.0 bar, with NH4I(s) but no HI(g) present?
(a) 8.5 bar
(b) 9.8 bar
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