A sample of sulfur hexafluoride gas occupies a volume of 9.10 L at 198ÁC. Assuming that the pressure remains constant, what temp
2 answers:
Temperature <u>-143.6°C</u> is needed to reduce the volume to 2.50 L
<h3>Further explanation </h3>There are several gas equations in various processes:
• 1. Avogadro's hypothesis
In the same temperature and pressure, in the same volume conditions, the gas contains the same number of molecules
So it applies: the ratio of gas volume will be equal to the ratio of gas moles
<h3>V1: V2 = n1: n2 </h3>• 2. Boyle's Law
At a fixed temperature, the gas volume is inversely proportional to the pressure applied
<h3>p1.V1 = p2.V2 </h3>• 3. Charles's Law
When the gas pressure is kept constant, the gas volume is proportional to the temperature
<h3>V1 / T1 = V2 / T2 </h3>• 4. Gay Lussac's Law
When the volume is not changed, the gas pressure in the tube is proportional to its absolute temperature
<h3>P1 / T1 = P2 / T2 </h3>• 5. Law of Boyle-Gay-Lussac
Combined with Boyle's law and Gay Lussac's law
<h3>P1.V1 / T1 = P2.V2 / T2 </h3>P1 = initial gas pressure (N / m2 or Pa)
V1 = initial gas volume (m3)
P2 = gas end pressure
V2 = the final volume of gas
T1 = initial gas temperature (K)
T2 = gas end temperature
In the problem, the conditions that are set constant are Pressure, so we use Charles' Law
V1 / T1 = V2 / T2
V1 = 9.1 L
T1 = 198 °C+273 = 471 K
V2 = 2.5 L
Then :
a description of Charles’s law
Charles's law
State Boyle's, Charles's, and Gay-Lussac's laws
Keywords : Charles Law, temperature, pressure, vollume, gas, sulfur hexafluoride
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Answer:
We need 0.375 mol of CH3OH to prepare the solution
Explanation:
For the problem they give us the following data:
Solution concentration 0,75 M
Mass of Solvent is 0,5Kg
knowing that the density of water is 1g / mL, we find the volume of water:
Now, find moles of are needed using the molarity equation:
therefore the solution is prepared using 0.5 L of H2O and 0.375 moles of CH3OH, resulting in a concentration of 0,75M