The equilibrium constant (Kp) is 0.16 at a particular temperature for the reaction:
N₂O₄(g) ⇌ 2NO₂(g)
Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the...
Lon Capa HW 12 - Chem 102 Questions
& Answers
The equilibrium constant (Kp) is 0.16 at a particular temperature for the reaction:
N₂O₄(g) ⇌ 2NO₂(g)
Given the following sets of initial conditions, what is the net change that must occur for
the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does
the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial
concentrations so no net change will occur?
a) P(NO₂) = 0.130 atm, P(N₂O₄) = 0.06 atm
b) P(NO₂) = ,0.145 atm P(N₂O₄) = 0.132 atm
c) P(NO₂) = 0.115 atm, P(N₂O₄) = 0.144 atm
d) P(NO₂) = 0.095 atm, P(N₂O₄) = 0.056 atm
e) P(NO₂) = 0.219 atm , P(N₂O₄) = 0.136 atm - ANSWERSa) left
b) equilibrium
c) right
d) equilibrium
e) left
The equilibrium constant is 0.090 at a particular temperature for the reaction:
H₂O(g) + Cl₂O(g) ⇌ 2HOCl(g)
Use this information to decide what will happen, given the following sets of initial
conditions: Will the reaction shift to the left, to the right or will the system be at
equilibrium?
a) A 3.0 L flask contains 0.58 mol H₂O, 0.0009 mol Cl₂O and 0.26 mol HOCl.
b) A 3.0 L flask contains 1.14 mol H₂O, 0.079 mol Cl₂O and 0.09 mol HOCl.
c) P(H₂O) = 453 torr, P(Cl₂O) = 13.2 torr, P(HOCl) = 23.2 torr
d) P(H₂O) = 196 torr, P(Cl₂O) = 63 torr, P(HOCl) = 24.8 torr - ANSWERSa) left
b) equilibrium
c) equilibrium
d) right
Consider the following reaction:
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