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3 years ago

What is the molarity of a solution prepared by dissolving 10.0g of kno3 in 250 ml of solution

Chemistry

1 answer:

maw [93]3 years ago

8 0

Answer:

Mass of KNO3= 10g

Molar mass of KNO3 = 101.1032g/mol

Volume = 250ml = 0.25L

No of mole on of KNO3 = mass of KNO3/Molar mass of KNO3

no of mole of KNO3 = 10/101.1032

No of mole of KNO3 = 0.09891

molarity of KNO3 = no of mole of KNO3/Vol (L)

Molarity = 0.09891/0.25 = 0.3956M

Molarity of KNO3 = 0.3956M

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Answer : The energy removed must be, 29.4 kJ

Explanation :

The process involved in this problem are :

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The expression used will be:

$Q=[m\times c_{p,l}\times (T_{final}-T_{initial})]+[m\times \Delta H_{fusion}]+[m\times c_{p,s}\times (T_{final}-T_{initial})]$

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$c_{p,l}$ = specific heat of liquid benzene = $1.73J/g^oC=1.73J/g.K$

$\Delta H_{fusion}$ = enthalpy change for fusion = $-9.8kJ/mol=-\frac{9.8\times 1000J/mol}{78g/mol}=-125.6J/g$

Now put all the given values in the above expression, we get:

$Q=[94.4g\times 1.73J/g.K\times (279-322)K]+[94.4g\times -125.6J/g]+[94.4g\times 1.51J/g.K\times (205-279)K]$

$Q=-29427.312J=-29.4kJ$

Negative sign indicates that the heat is removed from the system.

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