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  • (a)    Explain why on addition of 1 mol glucose to 1 litre water the boiling point of water increases. (b)    Henry’s law constant for CO2 in water is <img alt="1.67 \times 10^8 \text{ Pa}

(a)    Explain why on addition of 1 mol glucose to 1 litre water the boiling point of water increases.
(b)    Henry’s law constant for CO2 in water is 1.67 \times 10^8 \text{ Pa} at 298 K. Calculate the number of moles of CO2 in 500 ml of soda water when packed under 2.53\times 10^5 \text{ Pa}  at the same temperature.

 

 

 

 
 
 
 
 

Answers (1)

(a)    On addition of 1 mol glucose to 1 litre water, the boiling point of water increases because the addition of glucose decreases the vapour pressure of solution form, hence solution has to be heated to a temperature greater than the boiling point of pure solvent so as to make its vapour pressure equal to atmospheric pressure.

(b)    K_H = 1.67 \tiemes 10^8 \text{ Pa}

        P_{\mathrm{CO_2}} = 2.53\times 10^5 \test{ Pa}

        P_{\mathrm{CO_2}} = K_H X

        X = \frac{2.53\times 10^5}{1.67\times 10^8} = 1.5149\times 10^{-3} = 0.0015

        X = \frac{n_{\mathrm{CO_2}}}{n_{\mathrm{H_2O}}}

        n_{\mathrm{H_2O}} = \frac{500}{18} = 27.78 \ \mathrm{mol}

        0.0015 = \frac{n_{\mathrm{CO_2}}}{27.78}

        n_{\mathrm{CO_2}} = 0.04167

Quantity of CO2 in 500 ml soda water

                        0.04167\times 44

                        = 1.83348 \text g

Posted by

Sumit Saini

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