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olga2289 [7]
2 years ago
14

A balloon containing 0.0400 mol of a gas with a volume of 500 mL was expanded to 1.00 L. Answer the questions and round answers

to nearest hundredth place.
What is the final number of moles?
Chemistry
1 answer:
grandymaker [24]2 years ago
8 0

the number of moles 0.08

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Osmotic pressure is calculated by the product of the concentration in molarity, the  temperature, the vant Hoff factor (3 for CaCl2 and 1 for sucrose) and R, universal gas constant. At the same temperature, the osmotic pressures of both solutions are equal.

π = CRTi
For CaCl2,
π = (1)RT(3) = 3RT

For sucrose,
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Which of the following is a physical change?
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What is the initial temperature of a gas if the volume changed from 1.00 l to 1.10 l and the final temperature was determined to
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Using charles law
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Come up with a three-step plan for your household to reduce its effect on water pollution. Your plan should include a way to edu
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Part A Find ΔS∘ for the reaction between nitrogen gas and hydrogen gas to form ammonia: 12N2(g)+32H2(g)→NH3(g) Express your answ
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Answer:

\Delta S^{0} for the given reaction is -99.4 J/K

Explanation:

Balanced reaction: \frac{1}{2}N_{2}(g)+\frac{3}{2}H_{2}(g)\rightarrow NH_{3}(g)

\Delta S^{0}=[1mol\times S^{0}(NH_{3})_{g}]-[\frac{1}{2}mol\times S^{0}(N_{2})_{g}]-[\frac{3}{2}mol\times S^{0}(H_{2})_{g}]

where S^{0} represents standard entropy.

Plug in all the standard entropy values from available literature in the above equation:

\Delta S^{0}=[1mol\times 192.45\frac{J}{mol.K}]-[\frac{1}{2}mol\times 191.61\frac{J}{mol.K}]-[\frac{3}{2}mol\times 130.684\frac{J}{mol.K}]=-99.4J/K

So, \Delta S^{0} for the given reaction is -99.4 J/K

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