Moles and Stoichiometry

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# Moles and Stoichiometry - PowerPoint PPT Presentation

Moles and Stoichiometry. Regent Review. Correct Answer 0.5 moles. Correct Answer is 6. Correct Answer is (3) C 4 H 8. Correct Answer is (2) 1:2. (4) 310 g/mol is the correct answer. Moles = grams/ molar mass 20 grams/ 85 (g/mol) = .235 moles.

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### Moles and Stoichiometry

Regent Review

Moles = grams/ molar mass

• 20 grams/ 85 (g/mol) = .235 moles

• In equation 3, there are the same number of atoms on each side of the equation.  (Six atoms in the products and six atoms in the reactants.)

36 Which formula is both a molecular and an empirical formula?(1) C6H12O6    (3) C3H8O(2) C2H4O2     (4) C4H8

• Empirical is fully reduced to the simplest whole number ratio

10 The sum of the atomic masses of the atoms in one molecule of C3H6Br2 is called the(1) formula mass(2) isotopic mass(3) percent abundance(4) percent composition

• formula mass=mass of the formula

39 Which balanced equation represents a single replacement reaction?(1) Mg + 2AgNO3 → Mg(NO3)2+ 2Ag(2) 2Mg + O2 → 2MgO(3) MgCO3 → MgO + CO2(4) MgCl2+ 2AgNO3 → 2AgCl + Mg(NO3)2

• A+BC-->AC + B

35 Which equation represents a decomposition reaction?(1) CaCO3(s) ==>CaO(s) + CO2(g)(2) Cu(s) + 2AgNO3(aq)  ==>2Ag(s) + Cu(NO3)2(aq)(3) 2H2(g) + O2(g)  ==>2H2O(l)(4) KOH(aq) + HCl(aq)  ==>KCl(aq) + H2O(l)

• AB==> A + B

36 A compound has the empirical formula CH2O and a gram-formula mass of 60. grams per mole. What is the molecular formula of this compound?(1) CH2O         (3) C3H8O(2) C2H4O2        (4) C4H8O4

Given the equation:

__FeCl2 + __Na2CO3 → __FeCO3 + __NaClWhen the equation is correctly balanced using the smallest whole numbers, the coefficient of NaCl is

• 6
• 2
• 3
• 4

What is the percent by mass of oxygen in Fe2O3

(formula mass = 160)?

• 16%
• 30.%
• 56%
• 70.%

What is the correct formula for chromium (III) oxide?

• CrO3
• Cr3O
• Cr2O3
• Cr3O2

A hydrated salt is a solid that includes water molecules within its crystal structure. A student heated a 9.10-gram sample of a hydrated salt to a constant mass of 5.41 grams. What percent by mass of water did the salt contain?

• 3.69%
• 16.8%
• 40.5%
• 59.5%

Gypsum is a mineral that is used in the construction industry to make drywall (sheetrock). The chemical formula for this hydrated compound is CaSO4• 2 H2O. A hydrated compound contains water molecules within its crystalline structure. Gypsum contains 2 moles of water for each 1 mole of calcium sulfate.

• What is the gram formula mass of CaSO4• 2 H2O? Round your answer to the nearest whole number.
• Answer:  172 or 172.2 grams

Gypsum is a mineral that is used in the construction industry to make drywall (sheetrock). The chemical formula for this hydrated compound is CaSO4• 2 H2O. A hydrated compound contains water molecules within its crystalline structure. Gypsum contains 2 moles of water for each 1 mole of calcium sulfate.

• Calculate the percent composition by mass of water in this compound. Round your answer to the nearest percent.
• Answer:  21 or 20.9 or 20.93 %

Which pair of formulas correctly represents a molecular formula and its corresponding empirical formula?

• C2H2and CH
• C3H4 and CH2
• C4H6 and CH
• C5H8 and C2H2
• Correct Answer is C2H2 and CH