Chemistry: Enter your answer in the provided box. a sample of sulfur hexafluoride gas occupies 9.53 l at 215°c. assuming that the pressure remains constant, what temperature (in °c) is needed to reduce the volume to 4.36 l? report your answer to the proper number of significant figures.

That depends upon the body that you are talking about but usually the volume would go up as well. They are directly proportional....

Enter your answer in the provided box. a sample

Ответ:

dayanara72

15.03.2022

Chemistry

Explanation:

According to ideal gas equation, the product of pressure and volume equals to the product of number of moles, gas constant and temperature.

Mathematically, PV = nRT

Since, it is given that pressure is constant and Charle's law states that at constant pressure volume of an ideal gas is directly proportional to the absolute temperature.

Therefore, $V \propto T$

$\frac{V}{T}$ = constant

So, number of moles will also be constant then. Hence, the formula will be as follows.

$\frac{V_{1}}{T_{1}}$ = $\frac{V_{2}}{T_{2}}$

As it is given that $V_{1}$ is 9.53 L, $V_{2}$ is 4.36 L, $T_{1}$ is $215^{o}C$ that is also equal to (215 + 273) K = 488 K.

Now, putting these values into the formula as follows.

$\frac{V_{1}}{T_{1}}$ = $\frac{V_{2}}{T_{2}}$

$\frac{9.53 L}{488 K}$ = $\frac{4.36 L}{T_{2}}$

$T_{2}$ = 223.26 K

Temperature in degree celsius will be (223.26 K - 273 K) = $-49.73^{o}C$

Thus, we can conclude that temperature (in °C) is needed to reduce the volume to 4.36 L is $-49.73^{o}C$ .

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Enter your answer in the provided box. a sample of sulfur hexafluoride gas occupies 9.53 l at 215°c. assuming that the pressure remains constant, what temperature (in °c) is needed to reduce the volume to 4.36 l? report your answer to the proper number of significant figures.

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