IOM 2019, Експеримент — Задача 6. Exercise 1.6: Calculation of carbon dioxide solubility at room temperature

The 4th International Olympiad of Metropolises — Carbon Dioxide Solubility in Water

Условие

Write down a formula for the total number of carbon dioxide moles in the flask as the sum of the number of moles in the gas phase and in the dissolved state. For this purpose use the following notations: $V_w$ as the volume of water in the flask, $V$ as the volume of gas phase, $p$ as the equilibrium partial pressure of carbon dioxide above water, $T$ as the temperature of water and gas in the flask, $T_0 = 273.15\ \mathrm{K}$, $R$ as the universal gas constant, and $\alpha$ as the solubility of carbon dioxide in water.

Let's assume that during the experiment the total number of carbon dioxide moles in the flask is constant.

When the negative inlet of manometer is open, the pressure measured by the manometer is the difference between the pressure in the flask and the atmospheric pressure $p_a$. Write down a formula for the carbon dioxide partial pressure in the flask as a function of the manometer reading $\Delta p$. When deriving the formula, remember what the gas phase consists of. Calculate the product $pV$ (equilibrium pressure of carbon dioxide in the flask by the volume of its gas phase) versus the equilibrium pressure of carbon dioxide.

Draw a graph of the obtained relationship $pV(p)$. Calculate its slope.

Write down the water temperature in the box during the measurements. Remove the plug from the flask. Measure the volume of water in the flask using an electronic scale (take the water density as 1 g/cm$^3$). Calculate the carbon dioxide solubility on the basis of the graph slope and the obtained values of the box water temperature and the volume of water in the flask. Estimate the error of your measurements.

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Оригинал в Архива: phys-task-prak-iom-2019-en.pdf · официални решения: phys-solution-prak-iom-2019-en.pdf