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3 years ago

A 2.5 L container holds a sample of hydrogen gas at 291 K and 180 kPa.

Chemistry

1 answer:

netineya [11]3 years ago

6 0

Answer:

The new temperature will be 565.83 K.

Explanation:

Gay Lussac's law establishes the relationship between the temperature and the pressure of a gas when the volume is constant. This law says that the pressure of the gas is directly proportional to its temperature. This means that if the temperature increases, the pressure will increase; or if the temperature decreases, the pressure will decrease.

In other words, Gay-Lussac's law states that when a gas undergoes a constant volume transformation, the ratio of the pressure exerted by the gas temperature remains constant:

$\frac{P}{T} =k$

When an ideal gas goes from a state 1 to a state 2, it is true:

$\frac{P1}{T1} =\frac{P2}{T2}$

In this case:

P1= 180 kPa
T1= 291 K
P2= 350 kPa
T2= ?

Replacing:

$\frac{180 kPa}{291 K} =\frac{350 kPa}{T2}$

Solving:

$T2=350 kPa*\frac{291 K}{180 kPa}$

T2= 565.83 K

The new temperature will be 565.83 K.

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4.54 moles of H

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Why?

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To know the percent of each element, we need to to the following:

$C=\frac{72.08g}{176.138g}*100=0.409*100=40.92(percent)\\\\H=\frac{8.064g}{176.138g}*100=4.58(percent)\\\\O=\frac{95.994}{176.138g}*100=54.49(percent)$

So, we know that for the 100 grams of the compound, there are:

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4.58 grams of H

54.49 grams of O

We know the molecular masses of each element:

$C=12.0107\frac{g}{mol}\\\\H=1.008\frac{g}{mol}\\\\O=15.999\frac{g}{mol}{mol}$

Now, to calculate the number of moles of each element, we need to divide the mass of each element by the molecular mass of each element:

$C=\frac{40.92g}{12.010\frac{g}{mol}}=3.41mol\\\\H=\frac{4.58g}{1.008\frac{g}{mol}}=4.54mol\\\\O=\frac{54.49g}{15.999\frac{g}{mol}}=3.40mol$

Hence, we have that there are 3.41 moles of C, 4.54 moles of H, and 3.40 moles of O.

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