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Morgarella [4.7K]
3 years ago
6

Use the van der waals equation to calculate the pressure exerted by 1.335 mol of cl2 in a volume of 4.920 l at a temperature of

272.0 k .
Chemistry
1 answer:
nika2105 [10]3 years ago
7 0
<span>Van der waal or ideal eqn is given by PV = NRT; P = NRT/ V. Where N = 1.335 is the number of moles. T = 272K is temperature. V = 4.920L is the volume. And R = 0.08205L. Substiting the values into the eqn; we have, P = (1.331* 0.08205 * 272)/ 4.920 = 29.7047/ 4.920 = 6.03atm.</span>
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2 years ago
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Lilit [14]

Answer:

pH = 1.32

Explanation:

                 H₂M + KOH ------------------------ HM⁻ + H₂O + K⁺

This problem involves a weak diprotic acid which we can solve by realizing they amount  to buffer solutions.  In the first  deprotonation if all the acid is not consumed we will have an equilibrium of a wak acid and its weak conjugate base. Lets see:

So first calculate the moles reacted and produced:

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it is clear that the maleic acid will not be completely consumed, hence treat it as an equilibrium problem of a buffer solution.

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Using the Henderson - Hasselbach equation to solve for pH:

ph = pKₐ + log ( HM⁻/ HA) = 1.92 + log ( 0.015 / 0.059) = 1.325

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3 years ago
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saw5 [17]

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The net force on a vehicle that is accelerating at a rate of 1.2 m/s² is 1500 newtons. What is the mass
kotegsom [21]

Answer:

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