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What is the pressure, in atmospheres, of a 0.108-mol sample of helium gas at a temperature of 20.0°C if its volume is 0.505 L?
1 answer:
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<u>Answer:</u> The value of is coming out to be 0.412
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For
</u>
Given mass of = 1.00 kg = 1000 g (Conversion factor: 1 kg = 1000 g)
Molar mass of = 339.7 g/mol
Putting values in equation 1, we get:
- <u>For hydrogen gas:</u>
Given mass of hydrogen gas = 10.0 g
Molar mass of hydrogen gas = 2 g/mol
Putting values in equation 1, we get:
- <u>For hydrogen sulfide:</u>
Given mass of hydrogen sulfide = 72.6 g
Molar mass of hydrogen sulfide = 34 g/mol
Putting values in equation 1, we get:
The chemical equation for the reaction of antimony sulfide and hydrogen gas follows:
Initial: 2.944 5
At eqllm: 2.944-x 5-3x 2x 3x
We are given:
Equilibrium moles of hydrogen sulfide = 2.135 moles
Calculating for 'x', we get:
Equilibrium moles of hydrogen gas = (5 - 3x) = (5 - 3(0.712)) = 2.868 moles
Volume of the container = 25.0 L
Molarity of a solution is calculated by using the formula:
The expression of for above equation, we get:
The concentration of solids and liquids are not taken in the expression of equilibrium constant.
Hence, the value of is coming out to be 0.412