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Answer:
5.437L
Explanation:
If you convert 77.2°C to Kelvin you would add 273 that gives you 350.2K. Then it says standard temperature and pressure, which is 273° K and 760mmHg. I’m about 99% sure this is right! Sorry I hope this helps some!
Answer is: 5,75·10⁻¹.
Kf = 2,3·10⁶ 1/s.
K = 4,0·10⁸ 1/s.
Kr = ?
Kf - <span>forward rate constant.
K - </span><span>equilibrium constant.
Kr - </span><span>reverse rate constant.
</span>Since both Kf and Kr are constants at a given temperature, their ratio is also a constant that
is equal to the equilibrium constant K.<span>
K = Kf/Kr.
Kr = Kf/K = </span>2,3·10⁶ 1/s ÷ 4,0·10⁸ 1/s = 5,75·10⁻¹.
Van der Waals equation is as follows:
(P + a(n/V)²) * (V -nb) = n RT
Moles of H₂ is calculated by dividing 25 g by 2 (molecular weight of H₂) = 12.5 moles
Values of a and b are:
a = 0.02444 atm L² / mol
b = 0.0266 L / mol
(P + 0.02444 (12.5/1)²) * (1 -(12.5 *0.0266)) = 12.5 * 0.0821 * 293 K
If we solve this equation we get pressure of 412.29 atm
With ideal gas equation we get:
P V = n R T
P = n * R * T / V = (12.5 * 0.0821 * 293 / 1) = 300.69 atm