A mixture of gaseous hydrogen and gaseous iodine are in equilibrium with hydrogen iodide, as shown in the following equation.
H2 (g) + I2 (g) <=> 2HI (g)
Calculate the concentration of HI when the equilibrium constant is 1 x 105, the equilibrium concentration of H2 is 0.04M, and the equilibrium concentration of I2 is 0.009M.
Zinc carbonate dissolves in water to the extent of 1.12 x 10-4 g/L at 25 C. Calculate the solubility product Ksp for ZnCO3 at 25 C.
2 answers
Marcus, you should post your own question and not go piggy back on another. I mistook your post for a new question as an answer to Indigo's question. I'll do both here.
ZnCO3(s) ==> Zn^2+(aq) + [CO3^2-](aq)
(ZnCO3) = 1.12e-4 g/L or 1.12/molar mass ZnCO3 = 1.12/125.4 = 8.93E-7M
Ksp = (Zn^2+)(CO3^2-) = (8.93E-7)(8.93E-7) = ?
My calculator is on the blink so check the numbers very closely.
For the question by Marcus Z.
H2 (g) + I2 (g) <=> 2HI (g)
K = (HI)^2/(H2)(I2) = 1E5
The problem gives you H2 and I2 and K. Plug in those value and solve for the one unknown of HI. Post your work if you get stuck.
ZnCO3(s) ==> Zn^2+(aq) + [CO3^2-](aq)
(ZnCO3) = 1.12e-4 g/L or 1.12/molar mass ZnCO3 = 1.12/125.4 = 8.93E-7M
Ksp = (Zn^2+)(CO3^2-) = (8.93E-7)(8.93E-7) = ?
My calculator is on the blink so check the numbers very closely.
For the question by Marcus Z.
H2 (g) + I2 (g) <=> 2HI (g)
K = (HI)^2/(H2)(I2) = 1E5
The problem gives you H2 and I2 and K. Plug in those value and solve for the one unknown of HI. Post your work if you get stuck.
0 answers