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Aleks04 [339]
3 years ago
5

2. Rank the boiling points of methane, methanol, and methanal from lowest to highest. Explain your ranking. (6 points) 3. The lo

ne pair of electrons on the oxygen atom in an ester can form hydrogen bonds in some situations, but esters cannot form hydrogen bonds with each other. How would you expect the boiling point of an ester to compare with that of an alcohol
Chemistry
1 answer:
zlopas [31]3 years ago
6 0

Answer:

(2) Boiling point order: Methanol (highest) > Methanal > Methane (weakest)

(3) Boiling point of alcohol will be higher than ester molecules

Explanation:

(2) Methane is a non-polar molecule. Hence only weakest van der waal inter molecular force is present between methane molecules.

Methanal is polar molecule due to presence of polar aldehyde group. hence weaker dipole-dipole inter molecular force is present between methanal molecules.

Methanol is a polar protic molecule. Hence strongest H-bonding force act between methanol molecules.

The stronger the inter molecular force, the higher will be boiling point.

Boiling point order: Methanol (highest) > Methanal > Methane (weakest)

(3) An alcohol is a polar protic molecule. Hence strongest H-bonding force exist between alcohol molecules.

An ester is  polar molecule. Therefore weaker dipole-dipole inter molecular force is present between ester molecules.

So boiling point of alcohol will be higher than ester molecules.

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3 years ago
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Un globo lleno de helio tenia un volumen de 8.5 L en el suelo a 20°C y a una presión de 750 torr. Cuando se le soltó, el globo s
Ray Of Light [21]

Answer:

El volumen del gas era 12.95 L

Explanation:

Se relaciona la presión y el volumen mediante la ley de Boyle, que dice:

“El volumen ocupado por una determinada masa gaseosa a temperatura constante, es inversamente proporcional a la presión”

La ley de Boyle se expresa matemáticamente como:  P*V=k

Por otro lado, la Ley de Charles consiste en la relación que existe entre el volumen y la temperatura absoluta de una cierta cantidad de gas ideal, el cual se mantiene a una presión constante. Esta ley dice que cuando la cantidad de gas y de presión se mantienen constantes, el cociente que existe entre el volumen y la temperatura siempre tendrán el mismo valor:  

\frac{V}{T}=k

Por último, la Ley de Gay Lussac dice que la temperatura absoluta y la presión son directamente proporcionales. Es decir, cuando se mantiene todo lo demás constante, mientras suba la temperatura de un gas subirá también su presión. Y mientras la temperatura del gas baje, lo mismo ocurrirá con la presión:

\frac{P}{T}=k

Combinado las mencionadas tres leyes se obtiene:

\frac{P*V}{T} =k

Cuando se desean estudiar dos diferentes estados, uno inicial y una final de un gas, se puede aplicar:

\frac{P1*V1}{T1} =\frac{P2*V2}{T2}

Recordando que la temperatura debe usarse en grados Kelvin, conoces los siguientes datos:

  • P1: 750 torr
  • V1: 8.5 L
  • T1: 20°C= 293°K (siendo 0°C=273°K)
  • P2: 425 torr
  • V2: ?
  • T2: -20°C= 253 °K

Reemplazando:

\frac{750 torr*8.5 L}{293K} =\frac{425 torr*V2}{253 K}

Resolviendo:

V2=\frac{750 torr*8.5 L}{293K} *\frac{253 K}{425 torr}

V2= 12.95 L

<u><em>El volumen del gas era 12.95 L</em></u>

<u><em></em></u>

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