The equilibrium concentrations for the reaction below were found to be [AgNO3] = 0.0070 M and [Cu(NO3)2] = 0.48 M at a certain temperature.
2 AgNO3(aq) + Cu(s) ⇋ Cu(NO3)2(aq) + 2Ag(s)
Find the equilibrium constant, Kc, for the reaction
Would it be 9795.92?
[AgNO3] = 0.0070 M and [Cu(NO3)2] = 0.48 M at a certain temperature.
2 AgNO3(aq) + Cu(s) ⇋ Cu(NO3)2(aq) + 2Ag(s)
Find the equilibrium constant, Kc, for the reaction
Kc = [Cu(NO3)2]/[AgNO3)]^2 = (0.48)(0.0070)^2 = ?
Those are the digits I get on my calculator but I wouldn't use that as the answer. You have only two significant figures (s.f.) in those number;(0.48 and 0.070 therefore, you are allowed only 2 in the answer so I would report the number as 9.8E4 or 9.8 x 10^4.
yes
To find the equilibrium constant, Kc, for the reaction, we need to use the concentrations of the reactants and products at equilibrium.
The equilibrium constant expression (Kc) for the given reaction is as follows:
Kc = ([Cu(NO3)2] * [Ag]²) / ([AgNO3]² * [Cu])
In this expression, [Cu(NO3)2], [Ag], [AgNO3], and [Cu] represent the molar concentrations of the respective species at equilibrium.
Given the equilibrium concentrations: [AgNO3] = 0.0070 M and [Cu(NO3)2] = 0.48 M, we need to determine the concentration of [Cu] at equilibrium.
From the balanced chemical equation, we can see that 2 moles of AgNO3 produce 1 mole of Cu(NO3)2 and 2 moles of Ag. Therefore, the concentration of [Cu] at equilibrium will be half of the concentration of [AgNO3].
So, [Cu] = [AgNO3] / 2 = 0.0070 M / 2 = 0.0035 M.
Now we can substitute these concentrations into the equation for Kc:
Kc = (0.48 M * (0.0035 M)²) / ((0.0070 M)² * 0.0035 M)
Calculating this expression will give the value of Kc for the reaction at the given temperature.