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3 years ago

What is the specific heat of silicon if the temperature of a 4.11 g sample of silicon

Chemistry

1 answer:

monitta3 years ago

4 0

Answer:

The right solution is "0.7107 J/g°C".

Explanation:

The given values are:

Mass,

m = 4.11 g

Temperature,

ΔT = 3.8°C

Heat,

Q = 11.1 J

The specific heat of silicon will be:

⇒ $C=\frac{Q}{m \Delta T}$

On substituting the values, we get

⇒ $=\frac{11.1}{4.11\times 3.8}$

⇒ $=\frac{11.1}{15.618}$

⇒ $=0.7107 \ J/g^{\circ}C$

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4 years ago

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<u>Explanation:</u>

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$\text{Boiling point of solution}-\text{boiling point of pure solvent}=i\times K_b\times m$

$\text{Boiling point of solution}-\text{Boiling point of pure solvent}=i\times K_f\times \frac{m_{solute}\times 1000}{M_{solute}\times w_{solvent}\text{(in g)}}$ ......(1)

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i = Vant Hoff factor = 1 (for non-electrolytes)

$K_b$ = Boiling point elevation constant = $2.53^oC/m$

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$M_{solute}$ = Molar mass of solute = ? g/mol

$w_{solvent}$ = Mass of solvent = 200 g

Putting values in equation 1, we get:

$81.20-80.10=1\times 2.53\times \frac{10\times 1000}{M_{solute}\times 200}\\\\M_{solute}=\frac{1\times 2.53\times 10\times 1000}{1.1\times 200}\\\\M_{solute}=115g/mol$

Hence, the molar mass of solute is 115 g/mol.

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3 years ago