5.42.  State and explain Dalton’s law of partial pressures. Can we apply Dalton’s law of partial pressures to a mixture of carbon monoxide and oxygen?

<p><strong>5.42.&nbsp;Dalton's law of partial pressure:</strong> When two or more non-reacting gases are enclosed in a vessel, the total pressure of the gaseous mixture is equal to the sum of the partial pressures that each gas will exert when enclosed separately in the same vessel at constant temperature.</p><p>P= P1 + P2 + P3</p><p>Where, P is the total pressure of the three gases A, B, and C enclosed in a container. P1, P2 and P3 are the partial pressures of the three gases when enclosed separately in the same vessel at a given temperature one by one.</p><p>No, the law cannot be applied. Carbon monoxide and oxygen readily combine to form carbon dioxide. The law can be applied only to the non-reacting gases.</p><p>&nbsp;</p>

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