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Helen [10]
3 years ago
6

A 2.50-l volume of hydrogen measured at â196 °c is warmed to 100 °c. calculate the volume of the gas at the higher temperature

, assuming no change in pressure
Chemistry
1 answer:
ivann1987 [24]3 years ago
5 0

To solve this we assume that the hydrogen gas is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant pressure and number of moles of the gas the ratio T/V is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

T1 / V1 = T2 / V2

V2 = T2 x V1 / T1

V2 = (100 + 273.15) K x 2.50 L / (-196 + 273.15) K

<span>V2 = 12.09 L</span>

Therefore, the volume would increase to 12.09 L as the temperature is increased to 100 degrees Celsius.

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Answer:

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Answer:

0.33 mol/kg NH₃

Explanation:

Data:

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

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not affected?

Explanation:

pretty sure M / concentration isn't affected, only volume.

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Why was 1,2 dichlorobenzene used as the solvent for the diels alder reaction we performed in the lab?
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Answer:

1,2 dichlorobenzene was used as the solvent for the diels alder reaction: <em>because the co elimination part of the reaction needs high temp and a high boiling point solvent such as 1,2 dichlorobenzene</em>

Explanation:

Diels-Alder Reaction is a useful synthetic tool to prepare cyclohexane rings. It is a process, which occurs in a single step that consists of a cyclic redistribution of its electrons. The two reagents are bond together through a cyclic transition state in which the two new C-C bonds are formed at the same time. For this to occur, most of the time, it is necessary a high temperature and high-pressure conditions. Since 1,2 dichlorobenzene has a boiling point of 180ºC is a good solvent for this type of reactions.

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