Chemistry

Chemistry, 08.07.2019 05:00, 22iungj

Consider the equilibrium, n2(g) + 2o2(g) < > n2o4(g). calculate the equilibrium constant, kpif the equilibrium partial pressures are 0.431 atm for n2o4, 0.0867 atm for n2 and 0.00868 atm for o21.52 x 10-56.60 x 1041.75 x 10-3573

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Chemistry, 08.07.2019 23:30, joy8348

For the equilibrium, n2o4(g)< > 2no2(g), the equilibrium constant kp = 0.316. calculate the equilibrium partial pressure of no2 if the equilibrium partial pressure of n2o4(g) is 3.48 atm. 1.05 atm 1.10 atm 3.32 atm 0.301 atm

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Chemistry, 08.07.2019 23:30, ahicks2004

Consider the equilibrium, n2(g) + 2o2(g) < > n2o4(g). calculate the equilibrium constant, kp if the equilibrium partial pressures are 0.431 atm for n2o4, 0.0867 atm for n2 and 0.00868 atm for o2 6.60 x 104 1.75 x 10-3 573 1.52 x 10-5

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Chemistry, 22.08.2019 20:30, oliviablue7535

Given this reaction at equilibrium: n2o4 ↔ 2no2, calculate the equilibrium constant (kp) if the partial pressures of n2o4 and no2 are xid-560689_1 and xid-560688_1respectively. a. 1.61 b. 8.24 c. 0.00289 d. 0.621

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Chemistry, 24.08.2019 00:10, mdbar321

A) if the equilibrium concentration in the reaction 2no2 ⇌ n2o4 finds [n2o4]= 2.9x10-3 and [no2]= 4.2x10-3 find the equilibrium constant, k. b) given k, if 0.100 m of no2 reacts, what will be the concentraitions when the reaction gets to equilibrium? c) if to the equilibrium, from previous, we add 0.0500 m n2o4, calculate the equilibrium concentraitions. which direction did the reaction shift?

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Consider the equilibrium, n2(g) + 2o2(g) < > n2o4(g). calculate the equilibrium constant, kpi...

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