The pressure of a moist gas at $27°C$  is 0.04 atm. The volume of the container is doubled at the same temperature. The new pressure of the moist gas is _______ × 10^-1atm. (Nearest integer)

(Given: The vapour pressure of water at $27°C$  is 0.4 atm)

<p>Pressure of gas = pressure of moist gas – Vapour pressure of water</p><p>= 4 atm – 0.4 atm</p><p>= 3.6 atm</p><p>On doubling the volume, pressure of gas is halved :</p><p>Total pressure =&nbsp;<span class="mathml" contenteditable="false"> <math> <mrow> <mrow> <mo> (</mo> <mrow> <mfrac> <mrow> <mn>3</mn> <mo>.</mo> <mn>6</mn> </mrow> <mrow> <mn>2</mn> </mrow> </mfrac> <mo>+</mo> <mn>0</mn> <mo>.</mo> <mn>4</mn> </mrow> <mo>)</mo> </mrow> <mo>=</mo> <mn>2</mn> <mo>.</mo> <mn>2</mn> <mi>a</mi> <mi>t</mi> <mi>m</mi> </mrow> </math> </span></p>

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