The Solubility Product Constant for calcium bromide is > 1. If calcium bromide is dissolved in water you can say that the equilibrium concentrations of calcium and bromide ions are: ... ...A. High ...B. Moderate ...C. Low The solubility of calcium bromide in water is: ... ...A. High ...B. Moderate ...C. Low
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Ответ:
(1). If calcium bromide is dissolved in water you can say that the equilibrium concentrations of calcium and bromide ions are high.
(2). The solubility of calcium bromide in water is high.
Explanation:
We know that for a reaction its solubility product is equal to the product of concentration of ions present.
For example,![CaBr_{2} \rightarrow Ca^{2+} + 2Br^{-}](/tpl/images/0566/2772/1453e.png)
As it is given that for this reaction
> 1. Hence, the product of concentration of both these ions will be greater than 1 which means that products are favored.
Therefore, equilibrium concentrations of calcium and bromide ions are high.
Also, more is the number of these ions formed more will be the solubility of the compound (
).
As a result, the solubility of calcium bromide in water is high.
Ответ:
The work done on neon = -323 J
The internal energy change= -392.84 J
The heat absorbed by neon = -69.84 J
Explanation:
Step 1: Data given
Number of moles = 0.500 moles
Pressure = 1 atm
Temperature = 273 Kelvin
The pressure will change from 1.00 atm to 0.200 atm. The temperature changes from 273 to 210 Kelvin.
a) calculate the work done on neon
W = -P(V2-V1)
⇒ with P = the pressure = 0.1 atm
⇒ with V1 = the initial volume = nRTi /Pi
⇒ with V2 = the final volume = nRTf /Pf
W = -PnR((T2/P2) -(T1/P1))
⇒ with T2 = the final temperature = 210 K
⇒ with T1 = the initial temperature = 273 K
⇒ with P2 = the final pressure = 0.200 atm
⇒ with P1 = the initial pressure = 1.00 atm
W = -nR (210*(0.1/0.2) - 273*(0.1/1.00))
W = -nR*(105 - 27.3)
W= -(0.500)*(8.314)*(77.7)
W = -323 J
b) calculate the internal energy change
E = (3/2)*nRT
ΔE = Ef - Ei
ΔE =(3/2)*nR(T2-T1)
⇒ with n= number of moles = 0.500 moles
⇒ with T2 =the final temperature = 210 K
⇒ with T1 = the initial temperature = 273 K
ΔE = (3/2)*(0.5)*(8.314)(210-273)
ΔE = -392.84 J
c) Calculate the heat absorbed by neon
ΔE = q + W
q = ΔE -W
⇒ with ΔE = -392.84 J
⇒ with W = -323 J
q = -392.84 J -( -323 J)
q =-392.84 J + 323 J
q = -69.84 J