Aluminum metal and bromine liquid (red) react violently to make aluminum bromide (white powder). One way to represent this equilibrium is: 2 AlBr3() 2 Al(s) + 3 Br2(1)
We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K. the equilibrium constant for the reaction above.
1) 2 Al(s) + 3 Br2 = 2 AlBrz(s)
2) Al(s) + 3/2 Br2(1) AlBr3(s) K2 =
3) AlBrz(s) = Al(s) + 3/2 Br2(1) K3 =
Drag and drop your selection from the following list to complete the || (1K)12 x 12 1/K Consider the reaction: S(s) + O2(g) SO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K, and Kb for reactions a and b below:
a) 2 S(s) + 3 O2(g)
b) SO2(g) + 1/2O2(g) = 2 SO3(9) Ka SO3(9) Kb K=
Answers: 1
Chemistry, 21.06.2019 23:30, ashleyjaslin
Calculate the expected ph values of the buffer systems from the experiments (a, b,c, d), using the henderson- hasselbalch equation, ph-pka+log[a-]/[ha]. use for pka values carbonic acid= 6.37, and acetic acid= 4.75.
Answers: 2
Aluminum metal and bromine liquid (red) react violently to make aluminum bromide (white powder). One...
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