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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<u>Answer:</u> The percentage yield of water is 9.5 %
<u>Explanation:</u>
We are given:
Moles of hydrogen = 14 moles
Moles of oxygen = 10 moles
The chemical equation for the formation of water from hydrogen and oxygen follows:
By Stoichiometry of the reaction:
2 moles of hydrogen gas reacts with 1 mole of oxygen gas
So, 14 moles of hydrogen gas will react with = of oxygen gas
As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent
Thus, hydrogen gas is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
2 moles of hydrogen gas produces 2 moles of water
So, 14 moles of hydrogen gas will produce = of water
To calculate the percentage yield of water, we use the equation:
Experimental yield of water = 1.33 moles
Theoretical yield of water = 14 moles
Putting values in above equation, we get:
Hence, the percent yield of the water is 9.5 %.