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2. Determine the molecular formulas to which the following empirical formulas and molar masses pertain. SNH (188.35 g/mol) b. NPC12 (347.64 g/mol) C. CoC404 (341.94 g/mol) d. SN (184.32 g/mol)

2. Determine the molecular formulas to which the following empirical formulas and molar masses pertain. SNH (188.35 g/mol) b. NPC12 (347.64 g/mol) C. CoC404 (341.94 g/mol) d. SN (184.32 g/mol)

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Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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2. Determine the molecular formulas to which the following empirical formulas and molar masses pertain. SNH (188.35 g/mol) b. NPC₁2 (347.64 g/mol) C. CoC404 (341.94 g/mol) d. SN (184.32 g/mol) 3. Natural Rubidium has the average mass of 85.4678 and is composed of isotopes 85Rubidium (mass= 84.9117) and 87 Rubidium. The ratio of atoms 85Rb/87Rb in natural rubidium is 2.591. Calculate the mass of 87Rb. 4. Dimethyl nitrosamine, (CH3)2N20, is a carcinogenic substance that may be formed in foods, beverages or gastric juices from the reaction of nitrite ion with other substances. a. What is the molar mass of dimethyl nitrosamine? b. How many moles of dimethyl nitrosamine are present in 150 mg? c. What is the mass of 0.75 moles of dimethyl nitrosamine? d. How many atoms of hydrogen are in 1.25 mole of dimethyl nitrosamine? e. What is the mass of 2.0 x 106 molecules of dimethyl nitrosamine? f. What is the mass in grams of one molecule of dimethyl nitrosamine?
Transcribed Image Text:2. Determine the molecular formulas to which the following empirical formulas and molar masses pertain. SNH (188.35 g/mol) b. NPC₁2 (347.64 g/mol) C. CoC404 (341.94 g/mol) d. SN (184.32 g/mol) 3. Natural Rubidium has the average mass of 85.4678 and is composed of isotopes 85Rubidium (mass= 84.9117) and 87 Rubidium. The ratio of atoms 85Rb/87Rb in natural rubidium is 2.591. Calculate the mass of 87Rb. 4. Dimethyl nitrosamine, (CH3)2N20, is a carcinogenic substance that may be formed in foods, beverages or gastric juices from the reaction of nitrite ion with other substances. a. What is the molar mass of dimethyl nitrosamine? b. How many moles of dimethyl nitrosamine are present in 150 mg? c. What is the mass of 0.75 moles of dimethyl nitrosamine? d. How many atoms of hydrogen are in 1.25 mole of dimethyl nitrosamine? e. What is the mass of 2.0 x 106 molecules of dimethyl nitrosamine? f. What is the mass in grams of one molecule of dimethyl nitrosamine?
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