Consider the reaction: 2NO( g )+Br2( g )2NOBr( g ) K p =28.4 at 298 K In a react
ID: 892189 • Letter: C
Question
Consider the reaction:
2NO(g)+Br2(g)2NOBr(g) Kp=28.4 at 298 K
In a reaction mixture at equilibrium, the partial pressure of NO is 126 torr and that of Br2 is 159torr .
What is the partial pressure of NOBr in this mixture?
The following reaction
2H2S(g)2H2(g)+S2(g),Kc=1.67×107 at 800C
is carried out at the same temperature with the following initial concentrations: [H2S]=0.100M, [H2]=0.100M, and [S2]=0.00 M. Find the equilibrium concentration of S2.
the reaction in the Interactive Worked Example is carried out at a different temperature at which Kc = 0.055. This time, however, the reaction mixture starts with only the product, [NO] = 0.0100 M, and no reactants. Find the equilibrium concentrations of N2, O2, and NO at equilibrium.
Explanation / Answer
2NO(g)+Br2(g)2NOBr(g) Kp=28.4 at 298 K
PNO = 126
PBR2 = 159
Find NOBr in mixture
Kp = PNOBr^2 / (PBr2)(PNO^2)
28.4 = PNOBr^2 / (126*159)
PNO = 754 torr
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