Chemistry, 16.12.2020 23:40 mrashrafkotkaat
The water in the can was heated until it reached its boiling point. At the boiling point, the liquid water evaporated and steam was visible. What happened to the air in the can when the water boiled? Explain.
As the mouth of the can was dipped into the cold water, the water vapor inside the can cooled and condensed. How does this impact the pressure inside the can? How does this compare to the pressure outside the can? You may use a picture or diagram to help explain your answer.
Why was the temperature gradient important? In other words, why was it important to have a very hot can of water and a very cold water bath?
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The lattice enthalpy (formation of ionic solid from ions in the gas phase) for agcl(s) is -916 kj/mol and the hydration enthalpy (dissolution of gaseous ions into water) is -850 kj/mol. how much heat (in joules) is involved in forming 1l of saturated agcl solution (1.8 × 10-4 g / 100 ml water) by dissolving agcl(s)? assume solution volume does not change much upon dissolution. the equations are given below. ag+(g) + cl−(g) æ agcl(s)
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The water in the can was heated until it reached its boiling point. At the boiling point, the liquid...
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