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2 years ago

A mixture of 0.220 moles CO, 0.350 moles H2 and 0.640 moles He has a total

Chemistry

1 answer:

emmasim [6.3K]2 years ago

6 0

Answer:

P(H₂) = 0.8533 atm

Explanation:

n(CO) = 0.220 mole

n(H₂) = 0.350 mole

n(He) = 0.640 mole

_______________

∑ n = 1.210 moles

mole fraction => X(H₂) = 0.350/1.210 = 0.2892

Dalton's Law of Partial Pressures => P(H₂) = X(H₂)·P(ttl) = 0.2892(2.95 atm) = 0.8533 atm

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3 years ago

Solid NaI is slowly added to a solution that is 0.0079 M Cu+ and 0.0087 M Ag+.Which compound will begin to precipitate first?NaI

NeTakaya

Answer :

AgI should precipitate first.

The concentration of $Ag^+$ when CuI just begins to precipitate is, $6.64\times 10^{-7}M$

Percent of $Ag^+$ remains is, 0.0076 %

Explanation :

$K_{sp}$ for CuI is $1\times 10^{-12}$

$K_{sp}$ for AgI is $8.3\times 10^{-17}$

As we know that these two salts would both dissociate in the same way. So, we can say that as the Ksp value of AgI has a smaller than CuI then AgI should precipitate first.

Now we have to calculate the concentration of iodide ion.

The solubility equilibrium reaction will be:

$CuI\rightleftharpoons Cu^++I^-$

The expression for solubility constant for this reaction will be,

$K_{sp}=[Cu^+][I^-]$

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Now we have to calculate the concentration of silver ion.

The solubility equilibrium reaction will be:

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The expression for solubility constant for this reaction will be,

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3 years ago

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