Chapter 4 Evens

Chapter 4 Evens - 4.16 Because P is a constant, we can use...

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4.16 Because P is a constant, we can use 1 2 1 2 = V V T T , which gives 2 2 22.5 L ; 19.9 L. 291 K 258 K = = V V 4.24 Because P , V , and T change, we use the relation 1 1 2 2 1 2 = PV PV T T . Substituting for the appropriate values, we get 3 3 2 2 (0.958 atm)( ) (1.08 atm)(355 cm ) ; 382 cm . 310 K 296 K V V = = 4.52 The molar mass of nitroglycerin is 227.1 1 g mol - . All products are gases under these conditions, so the total amount of gas produced is the sum of the pressures of the individual gases; the pressure is independent of the type of gas. From the equation we can see that 29 mol of gas is produced for 4 mol of nitroglycerin detonated. We can use this information and the ideal gas equation to calculate the volume of gases produced (nit. = nitroglycerin): gas, total 1 1 1 454 g nit. 29 mol gas 4 mol nit. 227.1 g mol nit. 215 kPa (8.314 51 L kPa K mol )(548 K) 307 L - - - = = = n RT V P 4.54 To answer this, we need to know the number of moles of 2 4 C H (g) present in each case. Because the combustion reaction is the same in both cases, as are the temperature and pressure, the larger number of moles of 2 4 C H (g)
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This note was uploaded on 04/08/2008 for the course CHEM CHEM 6B taught by Professor Christinajohnson during the Fall '07 term at UCSD.

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Chapter 4 Evens - 4.16 Because P is a constant, we can use...

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