CM-UY 1004 Lecture Notes - Lecture 5: Unified Atomic Mass Unit, Chemical Formula, Molecular Mass

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25 Sep 2017

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8 60 g of c h o. Molecular mass: sum of atomic masses (in amu) in a molecule. Smaller molar mass= greater number of moles. Assume 100 grams convert grams to moles by dividing my molar mass divide by smallest number of molecules empirical formula divide molar mass by mass of empirical formula for multiplier molecular formula. Chemical reaction: process where 1+ substances are changed into 1+ new substances. Chemical equation: uses chemical symbols to show what happens during a chemical.

Related Questions

I don't understand question 7 can you please help.

1) How many atoms are there in 51.3 g of barium chloride (BaCl2)?
2) How many moles of carbon monoxide (CO) are in 29.3 g of the compound?

3) What is the formula for copper(II) phosphate? Capitalization and punctuation count?

4) How many atoms of phosphorus are in 2.90 mol of copper(II) phosphate?

5) How many moles of N are in 0.191 g of N2O?

6) A sample of C3H8 has 7.68 Ã 1024 H atoms. How many carbon atoms does the sample contain? What is the total mass of the sample?

7) Calculate the percent composition by mass of each element in Al(OH)3. Use at least three significant figures.

% Al= ?, % O=? , % H =?

8) What is the empirical formula of a compound composed of 3.25% hydrogen (H), 19.36% carbon (C), and 77.39% oxygen (O) by mass?

HCO (Insert subscripts as needed.)

9) A compound with the empirical formula CH2 has a molar mass of 98 g/mol. What is the molecular formula for this compound?

CM-UY 1004 Lecture Notes - Lecture 5: Unified Atomic Mass Unit, Chemical Formula, Molecular Mass

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