By Martin Silberberg
Via Patricia Amateis of Virginia Tech. This complement includes specific recommendations and causes for all even-numbered difficulties often textual content. .
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Additional resources for Student Solutions Manual to accompany Principles of General Chemistry
The correct formula for this ionic compound is C U2CO). M of C u2C 03 = (2 x 63 . 5 5 ) + 1 2 . 0 1 + (3 x 1 6 . 00) = 1 8 7 . 4 1 mol C U 2 C03 ) ( 1 8 7 . 1 1 g Cu 2 CO 3 I mol C U 2 C03 ) = 1 5 7 3 . 57 x 3 1 0 g CU 2 C03 b ) D i n i trogen pentaox ide has the formula N20S ' Di- indicates 2 N atoms and penta- i ndicates 5 ° atoms. M of N20s = ( 2 x 1 4 . 00) = 1 08 . 02 gimol M ass N20S = ( 2 . 04 X 10 21 N 2 0S mOlecu les = 0 . 366 g N 2 0S ) [ 34 1 �3O l N 2 0S 6 . 02 2 x 1 0 N 2 0S molecules J( 1 08 .
If it is not obvious that the value is near 5/3 , use a trial and error procedure whereby the value is multiplied by the successively larger integer until a value near an integer results. This gives C S H 3 as the empirical formula. 000. Thus, the empirical formula must be multiplied by 4 to give C 2oH1 2 as the molecular formula of benzo[a]pyrene. 296 glmo!. This is very close to the given value. 6 Plan: The carbon in the sample is converted to carbon dioxide, the hydrogen is converted to water, and the remaining material is chlorine.
98 m o l c l. 3 . 540936 x 10 spla 24 . 5 ) X ( ( I mol ci splatin . J( . 300. 1 g clsp latm 6 mol H . 1 mol clsplatm 1 0 24 H atoms J 6 . 02 2 . · I atm = 0 . 950683 1 = 0 . 950 7 mo I CISP x 10 23 H 1 mol H atoms ) Plan: Determine the formulas for the compounds where needed. Determine the molar mass of each formula. Calculate the percent nitrogen by dividing the mass of nitrogen i n a mo l e of compound by the molar mass of the compound, and multiply the result by 1 00%. Then rank the values.