This worksheet is due on There will be no exception checked so do your work as a

Question

This worksheet is due on There will be no exception checked so do your work as accurately as possible. If the sheet is complete with all work included, will be worth 7 points the final exam. Let me if you have any questions. Please do the problems on another piece of paper What would the air pressure need be (give a specific numerical value) in to order for water to boil at room temperature? Explain how you determined your answer. As gas molecules are added to a rigid container, would the temperature need to be increased, decreased, or unchanged in order to keep the pressure constant? Explain using only kinetic-molecular theory. (That means do not use any equations.) Consider the following chemical reaction: 2 NO_2 (g) + 7 H_2(g) righarrow 2 NH_3(g) + 4 H2O(g) If 54.67 liters of hydrogen are used up (measured at 288 degree C and 1.39 atm) then what volume of water vapor is produced (measured at the same temperature and pressure)?

Explanation / Answer

1) The air pressure always should be equals to atmospheric pressure (1 atm) to boil water at 1000C

2) The temperature to be decreased as the pressure of the container increases because of addition of gas molecules.

3) Number of moles of hydrogen = (1.39 atm)(54.67 L) / (0.0821 L.atm/mol.K)(561 K) = 1.65 mol

Therefore, number of moles of H2O produced = (1.65 mol)(4/7) = 0.942 mol

Volume of H2O = (0.942 mol)(0.0821 L.atm/mol.K)(561 K) / 1.39 atm = 31.24 L

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