7) A flask that can withstand an internal pressure of 2500 torr, but no more, is filled with a gas at 21.0oC and 758 torr and heated. At what temperature will it burst? 8) A glass vessel contains 28 g nitrogen gas. Assuming ideal behavior, which of the processes listed below would double the pressure exerted on the walls of the vessel? a) Adding enough mercury to fill one-half the container. b) Raising the temperature of the container from 30. o C to 60. o C. c) Raising the temperature of the container from -73 o C to 127 o C.
CHEM111 Week 5 discussion questions d) Adding 28 g nitrogen gas (inert gas). Processes a, c, and d will all result in a doubling of the pressure. Process a has the effect of halving the volume, which would double the pressure (Boyle’s law). Process c doubles the pressure because the absolute temperature is doubled (from 200. K to 400. K). Process d doubles the pressure because the moles of gas are doubled (28 g N 2 is 1 mol of N 2 ). Process b won’t double the pressure since the absolute temperature is not doubled (303 K to 333 K). 9) Nitroglycerine, the explosive ingredient in dynamite, decomposes violently when shocked to form three gasses (N 2 , CO 2 , O 2 ) as well as water: C 3 H 5 (NO 3 ) 3 (l) → N 2 (g) + CO 2 (g) + O 2 (g) + H 2 O(l) a) Balance this equation b) Calculate how many moles of each gas are created in the explosion of 1kg of nitroglycerine. c) What volume would these gasses occupy at 1.0 atm? d) What are the partial pressures of each gas under these conditions? a) 4C 3 H 5 (NO 3 ) 3 (l) → 6N 2 (g) + 12CO 2 (g) + O 2 (g) + 10H 2 O(l) b) Molar Masses: C 3 H 5 (NO 3 ) 3 :227.09 g/mol N 2 , CO 2 , O 2 , H 2 O: Not needed Moles of C 3 H 5 (NO 3 ) 3 (l): (1000. g)(1 mol C 3 H 5 (NO 3 ) 3 /227.09 g) = 4.40 mol CO 2 : (4.40 mol C 3 H 5 (NO 3 ) 3 )(12 mol CO 2
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