Use the References to access important values if needed for this question. The v

Question

Use the References to access important values if needed for this question. The vapor pressure of liquid acetone. CH_3COCH_3. is 40.0 mm Hg at 264 K. A sample of CH3COCH3 is placed in a closed, evacuated container of constant volume at a temperature of 422 K. It i found that all of the CH_3COCH_3 is in the vapor phase and that the pressure is 71.0 mm Hg. If the temperature in the container is reduced to 264 K, which of the following statements are correct? Choose all that apply. Liquid acetone will be present. The pressure in the container will be 44.4 mm Hg. Some of the vapor initially present will condense. No condensation will occur. Only acetone vapor will be present. more group attempts remaining

Explanation / Answer

Use the ideal gas equation to determine how many moles of CH3OHCH3 you have

PV = nRT and n = PV/RT

Now first for P= 71 mmHg = 0.0934 atm and T= 422 K

Number of mole for acetone

n = 0.0934 atm x 1 L / (0.0821 L-atm/deg-mole)(422 K) = 0.00269 mol

Now second for P= 40 mmHg = 0.053 atm and T= 264 K

Number of mole for acetone

n = 0.053 atm x 1 L / (0.0821 L-atm/deg-mole)(264 K) = 0.00245 mol

so mole of acetone is decrease means Liquid acetone will be present

Now third for P= 44.4 mmHg = 0.05842 atm and T= 264 K

n = 0.05842 atm x 1 L / (0.0821 L-atm/deg-mole)(264 K) = 0.00269 mol

so the for constant volume, the pressure in the container will be 44.4 mmHg

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