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adelina 88 [10]
3 years ago
7

If the volume and moles of a container are held constant, the temperature of a gas is inversely proportional to the pressure.

Chemistry
1 answer:
noname [10]3 years ago
4 0

Answer:

FALSE

Explanation:

Assuming that the gas is ideal

Therefore the gas obeys the ideal gas equation

<h3>Ideal gas equation is </h3><h3>P × V = n × R × T</h3>

where

P is the pressure exerted by the gas

V is the volume occupied by the gas

n is the number of moles of the gas

R is the ideal gas constant

T is the temperature of the gas

Here volume of the gas will be the volume of the container

Given the volume of the container and number of moles of the gas are constant

As R will also be constant, the pressure of the gas will be directly proportional to the temperature of the gas

P ∝ T

∴ Pressure will be directly proportional to the temperature

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Answer: The value of K_{b} for chloroform is 3.62^{o}C/m when 0.793 moles of solute in 0.758 kg changes the boiling point by 3.80 °C.

Explanation:

Given: Moles of solute = 0.793 mol

Mass of solvent = 0.758

\Delta T_{b} = 3.80^{o}C

As molality is the number of moles of solute present in kg of solvent. Hence, molality of given solution is calculated as follows.

Molality = \frac{no. of moles}{mass of solvent (in kg)}\\= \frac{0.793 mol}{0.758 kg}\\= 1.05 m

Now, the values of K_b is calculated as follows.

\Delta T_{b} = i\times K_{b} \times m

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i = Van't Hoff factor = 1 (for chloroform)

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Substitute the values into above formula as follows.

\Delta T_{b} = i\times K_{b} \times m\\3.80^{o}C = 1 \times K_{b} \times 1.05 m\\K_{b} = 3.62^{o}C/m

Thus, we can conclude that the value of K_{b} for chloroform is 3.62^{o}C/m when 0.793 moles of solute in 0.758 kg changes the boiling point by 3.80 °C.

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Explanation:

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