It is calculated that 0.014 moles of oxygen (O₂) are present in the given sample by using the ideal gas law.
Calculation:
Provided that :
Temperature, T = 273+11 K = 284 K
Pressure, P = 0.5 atm
Volume, V = 0.65 L
Ideal gas constant,R = 0.08205 L atm/mol K
According to the ideal gas law,
we know the formula, PV = nRT
or, n = PV / RT = (0.5 * 0.65) / (0.08205 * 284)
or, n = 0.0139 ≈ 0.014 mole
What is the ideal gas law?
- The universal gas equation, often known as the ideal gas law, is the formula of state for a fictitious ideal gas. Although it has several restrictions, it is a decent approximation of the behavior of numerous gases under various circumstances.
- Benoît Paul Émile Clapeyron introduced it for the first time in 1834 as a synthesis of the experimental Boyle's law, Charles' law, Avogadro's law, and Gay-Lussac's law.
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Hey there!:
SO2 a Bent molecular shape. The lone pair of electrons is at the top of the SO2 molecule. The SO2 bond angle will be 120 degrees since it has a Bent molecular geometry.
Hope that helps!
This is an incomplete question, here is a complete question.
The Henry's law constant for oxygen dissolved in water is 4.34 × 10⁹ g/L.Pa at 25⁰C.If the partial pressure of oxygen in air is 0.2 atm, under atmospheric conditions, calculate the molar concentration of oxygen in air-saturated and oxygen saturated water.
Answer : The molar concentration of oxygen is, 
Explanation :
As we know that,
where,
= molar solubility of 
= ?
= partial pressure of = 0.2 atm = 1.97×10⁻⁶ Pa
= Henry's law constant = 4.34 × 10⁹ g/L.Pa
Now put all the given values in the above formula, we get:
Now we have to molar concentration of oxygen.
Molar concentration of oxygen = 
Therefore, the molar concentration of oxygen is,
Answer:
hope the inserted image will help :)
Explanation:
