Answer:
![\large\boxed{\large\boxed{K_c=\dfrac{[Cu^{2+}]}{[Ag^+]^2}}}](https://tex.z-dn.net/?f=%5Clarge%5Cboxed%7B%5Clarge%5Cboxed%7BK_c%3D%5Cdfrac%7B%5BCu%5E%7B2%2B%7D%5D%7D%7B%5BAg%5E%2B%5D%5E2%7D%7D%7D)
Explanation:
<u>1. Chemical equilibrium equation:</u>
<u>2. Species</u>
In an equilibrium constant expression you do not include the solid substances; only gases and dissolved substances.
The symbol 
means solid, thus Cu(s) and Ag(s) shall not appear in your equilibrium constant expression.
The symbol 
means in aqueous solution, thus the both 
and 
must appear in the equilibrium constant expression.
<u>3. Equilibrium constant expression.</u>
It is the quotient of the product of the concentrations of the species on the right hand side of the equilibrium equation, each raised to its corresponding coefficient, and the product of the concentrations of the species on the left hand side, each raised to its coresponding coefficient.
![K_c=\dfrac{[Cu^{2+}]}{[Ag^+]^2}](https://tex.z-dn.net/?f=K_c%3D%5Cdfrac%7B%5BCu%5E%7B2%2B%7D%5D%7D%7B%5BAg%5E%2B%5D%5E2%7D)
Answer:
The energy change in a chemical reaction is due to the difference in the amounts of stored chemical energy between the products and the reactants. This stored chemical energy, or heat content, of the system is known as its enthalpy.
Explanation:
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FeSO₄*7H₂O(s) = FeSO₄(s) + 7H₂O(g)
M(FeSO₄*7H₂O)=278.0 g/mol
M(FeSO₄)=151.9 g/mol
m(FeSO₄*7H₂O)/M(FeSO₄*7H₂O)=m(FeSO₄)/M(FeSO₄)
m(FeSO₄)=M(FeSO₄)m(FeSO₄*7H₂O)/M(FeSO₄*7H₂O)
m(FeSO₄)=151.9*100.0/278.0=54.6 g
m(FeSO₄)=54.6 g
Basis: 100 mL solution
From the given density, we calculate for the mass of the solution.
density = mass / volume
mass = density x volume
mass = (1.83 g/mL) x (100 mL) = 183 grams
Then, we calculate for the mass H2SO4 given the percentage.
mass of H2SO4 = (183 grams) x (0.981) = 179.523 grams
Calculate for the number of moles of H2SO4,
moles H2SO4 = (179.523 grams) / (98.079 g/mol)
moles H2SO4 = 1.83 moles
Molarity:
M = moles H2SO4 / volume solution (in L)
= 1.83 moles / (0.1L ) = 18.3 M
Molality:
m = moles of H2SO4 / kg of solvent
= 1.83 moles / (183 g)(1-0.983)(1 kg/ 1000 g) = 588.24 m
