Lecture 9 Supplement

Lecture 9 Supplement - Sample Question...

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Sample Question According to the chemical equation: how much NO 2 can be produced by the reaction of excess O 2 with 50.0 g of NO? the actual yield of NO 50.0 g, what is the % yield? (N=14 mu O=16 u If the actual yield of NO 2 is 50.0 g, what is the % yield? (N 14 amu,O16 amu) 50.0 g 1 mol 1 mol x g ? (molar relationship) g mol mol g g 67 . 1 / 30 0 . 50 mol mol g g 67 . 1 / 46 olar relationship) g mol mol g 7 . 76 666663 . 76 ) 67 . 1 ( ) / 46 ( (molar relationship) % 2 . 65 7 . 76 / 0 . 50 % g g yield
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How many grams of He must be added to a balloon containing 8.00 g He to double s volume? (He atom mass = 4 u T held constant) its volume? (He atom mass 4 amu, P, T held constant) He ( g )H e ( g ) 2 V l g 0 00 . 8 .00g g? V 1 V 2 =2 V 1 Avogadro’s Law mol mol g n 00 . 2 / 003 . 4 1 n 1 n 2 8.00g X g ? 1 1 n V 2 1 V V 1 1 n V 2 2 n V 2 1 n n 2 1 2 n V mols n n 00 . 4 00 . 2 2 2 1 2 2 1 2 1 1 2 1 V V n n g mol g mols mol g n X 16 / 00 . 4 00 . 4 / 00 . 4 2 So, 8.00 g of He must be added to double the volume
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Seven moles of carbon dioxide are stored in a 30.0-L container at 70 o C. What id the pressure in the container? =300L =70 + 273 = 343 K =7mo ls V = 30.0 L T = 70 o C + 273 = 343 K n = 7 mols R = 0.0821 L . atm/mol . K
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This note was uploaded on 03/07/2012 for the course 830 201 taught by Professor Leyton during the Fall '08 term at Rutgers.

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Lecture 9 Supplement - Sample Question...

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