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matrenka [14]
3 years ago
6

An ethylene glycol solution contains 16.2 g of ethylene glycol (c2h6o2) in 85.4 ml of water. calculate the boiling point of the

solution. calculate the freezing point of the solution. (assume a density of 1.00 g/ml for water.)
Chemistry
1 answer:
Andre45 [30]3 years ago
7 0
<span>Answer: (16.2 g C2H6O2) / (62.0678 g C2H6O2/mol) / (0.0982 kg) = 3.9704 mol/kg = 3.9704 m a.) (3.9704 m) x (1.86 °C/m) = 7.38 °C change 0.00°C - 7.38 °C = - 7.38 °C b.) (3.9704 m) x (0.512 °C/m) = 2.03 °C change 100.00°C + 2.03 °C = 102.03 °C</span>
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2 years ago
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serious [3.7K]

im pretty sute the answer would be number 4.

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2 years ago
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How molecules of N2 gas can be present in a 2.5 L flask at 50°C and 650 mmHg?
ratelena [41]

Answer:

0.482 ×10²³ molecules

Explanation:

Given data:

Volume of gas = 2.5 L

Temperature of gas = 50°C (50+273 = 323 k)

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Molecules of N₂= ?

Solution:

PV= nRT

n = PV/RT

n = 0.86 atm × 2.5 L /0.0821 atm. mol⁻¹. k⁻¹. L × 323 k

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5 0
3 years ago
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KengaRu [80]

Answer:

The answers are either 1 or 4

Explanation:

I am pretty dure it is 1

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This should help.
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