Question
In: Chemistry
The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH4I(s) <----> NH3(g)...
The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K.
NH4I(s) <----> NH3(g) + HI(g)
An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.308 mol NH4I, 8.37×10-3 M NH3 and 8.37×10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.50×10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished?
[NH3]=
[HI]=
Solutions
Expert Solution
NH4I(s) <----------------------------------> NH3(g) + HI(g)
0.308 8.37x 10^-3 8.37×10-3 M -----------------> equilibrium
[NH3] concentration changed to 1.50×10-2 M that means new concentrations of NH3 and HI are 1.50×10-2 M
concentrations of the two gases once equilibrium has been reestablished
[NH3] = 1.50×10-2 M
[HI] = 1.50×10-2 M
queen_honey_blossom answered 1 hour agoRelated Solutions
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The equilibrium constant, K, for the following reaction is
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An equilibrium mixture of the three gases in a 1.00 L flask at
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HI, 4.32×10-2 M
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I2. What will be the concentrations of
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3.12×10-2 mol of
I2(g) is added to the flask?
[HI]
=
M
[H2]
=
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[I2]
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An equilibrium mixture of the three gases in a 1.00 L flask at
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=
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[I2]
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