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Pepsi [2]
2 years ago
5

A certain liquid X has a normal boiling point of 133.60°C and a boiling point elevation constant Kb= 2.46°C kg mol^-1.Calculate

the bolling point of a solution made of 52.2g of benzamide (C7H7NO) dissolved in 350. g of X.
Chemistry
1 answer:
Afina-wow [57]2 years ago
6 0

Answer:

136.63 °C

Explanation:

ΔTb=Tb solution - Tb pure

Where; Tb pure = 133.60°C

molar mass of solute = 121.14 g/mol

number of moles of solute; 52.2g/121.14 g/mol = 0.431 moles

molality = 0.431 moles/350 * 10^-3 = 1.23 molal

Then;

ΔTb = Kb * m * i

Kb = 2.46°C kg mol^-1

m = 1.23 molal

i = 1

ΔTb = 2.46 * 1.23 * 1

ΔTb = 3.03 °C

Hence;

Tb solution = ΔTb + Tb pure

Tb solution = 3.03 °C + 133.60°C

Tb solution = 136.63 °C

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light energy is converted to chemical energy during photosynthesis.

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3 0
2 years ago
A 0.2722 g sample of a pure carbonate, X n CO 3 ( s ) , was dissolved in 50.0 mL of 0.1200 M HCl ( aq ) . The excess HCl ( aq )
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Answer:

0.00369 moles of HCl react with carbonate.

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According to above equation, 1 mol of NaOH reacts with 1 mol of 1 mol of HCl.

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3 0
3 years ago
It is desired to produce 2.25 grams of dichloromethane (CH2Cl2) by the following reaction. If the percent yield of dichlorometha
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