Please show work and explain! I need to know this stuff for a test! My teacher just doesn't teach us..
1. 2SO3(g)-> 2SO2 (g) + O2 (g)
Calculate K(eg) for this reaction if the equilibrium concentrations are:
[SO2] = 0.42M
[O2] = 0.21M
[SO3] = 0.072M
2. Will a precipitate form when 0.00070 mol Na2CO3 is mixed with 0.0015 mol Ba(OH)2 in one liter of solution? Assume that these two salts both dissolve completely.
I probably sound so stupid! haha they are probably too easy to figure out, am i right? ugh, please help!
1. 2SO3(g)-> 2SO2 (g) + O2 (g)
Calculate K(eg) for this reaction if the equilibrium concentrations are:
[SO2] = 0.42M
[O2] = 0.21M
[SO3] = 0.072M
2. Will a precipitate form when 0.00070 mol Na2CO3 is mixed with 0.0015 mol Ba(OH)2 in one liter of solution? Assume that these two salts both dissolve completely.
I probably sound so stupid! haha they are probably too easy to figure out, am i right? ugh, please help!
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Equilibrium Expression is K= [Product]^x[Product]^z / [Reactant]^y [Reactant]^w
x, z, y, and w are the coefficients from the reaction. Only aqueous and gasses matter.
So, (.21 * .42^2)/(.072 ^2) = K
2. 1As are always soluble so NaOH does not precipitate. BaCO3 does because CO3s are never soluble (except with 1As and NO3s).
x, z, y, and w are the coefficients from the reaction. Only aqueous and gasses matter.
So, (.21 * .42^2)/(.072 ^2) = K
2. 1As are always soluble so NaOH does not precipitate. BaCO3 does because CO3s are never soluble (except with 1As and NO3s).