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3 years ago

How many moles of gas would occupy a 25.0 liter when the temp is 22.0 degrees celsius and the pressure is 646 torr

Chemistry

1 answer:

Luda [366]3 years ago

3 0

Answer:

0.877 mol

Step-by-step explanation:

We can use the Ideal Gas Law to solve this problem.

pV = nRT Divide both sides by RT

n = (pV)/(RT)

Data:

p = 646 torr

V = 25.0 L

R = 0.082 06 L·atm·K⁻¹mol⁻¹

T = 22.0 °C

Calculations:

(a) Convert the pressure to atmospheres

p = 646 torr × (1 atm/760 torr) = 0.8500 atm

(b) Convert the temperature to kelvins

T = (22.0 + 273.15) K = 295.15 K

(c) Calculate the number of moles

n = (0.8500 × 25.0)/(0.082 06 × 295.15)

= 0.877 mol

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Which has the highest boiling point .33 m NH3 or .10 m Na2SO4

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Answer:

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Explanation:

Data:

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The formula for the boiling point elevation ΔTb is

$\Delta T_{b} = iK_{b}b$

i is the van’t Hoff factor — the number of moles of particles you get from a solute.

(a) For NH₃,

The ammonia is a weak electrolyte, so it exists almost entirely as molecules in solution.

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