An equilibrium mixture of pcl5(g), pcl3(g), and cl2(g) has partial pressures of 217.0 torr, 13.2 torr, and 13.2 torr, respectively. a quantity of cl2(g) is injected into the mixture, and the total pressure jumps to 263.0 torr (at the moment of mixing). the system then re-equilibrates. the appropriate chemical equation is pcl3(g)+cl2(g) < --> pcl5(g) calculate the new partial pressures after equilibrium is reestablished in torr

answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.

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