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Lecture 9 Supplement

# Lecture 9 Supplement - Sample Question howmuchNO2...

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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? If the actual yield of NO 2 is 50.0 g, what is the % yield? (N=14 amu, O=16 amu) is 50.0 g, what is the % yield? (N 14 amu, O 16 amu) 50.0 g 1 mol 1 mol x g ? (molar relationship) mol mol g g 67 . 1 / 30 0 . 50 mol mol g g 67 . 1 / 46 (molar relationship) g mol mol g 7 . 76 666663 . 76 ) 67 . 1 ( ) / 46 ( % 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 its volume? (He atom mass = 4 amu P T held constant) (He atom mass 4 amu, P, T held constant) He ( g ) He ( g ) V 1 V 2 =2 V 1 l g 00 2 00 . 8 8.00g X g ? Avogadro’s Law mol mol g n . / 003 . 4 1 n 1 n 2 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
Seven moles of carbon dioxide are stored in a 30.0-L container at 70 o C. What id the pressure in the container? V = 30 0 L T = 70 o C + 273 = 343 K n = 7 mols V = 30.0 L R = 0.0821 L . atm/mol . K PV = nRT atm V nRT P 57 . 6 0 30 343 0821 . 0 7 V nRT P . Seven moles of carbon monoxide under the same condition will have a

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