General Chemistry Chapter 3 and 4 multiple questions.

Chapter3:
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1. How many moles are in 3.01×10²³ atoms of Rb?

2. How many atoms are in 54.0 g of Al?

3. Determine the mass (g) of 0.120 mol of C₆H₁₂O₆.

4. Determine the percent of C in Na₂C₂O₄.

5. Determine the empirical formula for a compound composed of 34.6 % C, 3.9 % H, and 61.5 % O.

6. A compound composed of 41.39% C, 3.47% H, and 55.14% O. The molar mass of the compound is 116.07 g/mol. What is the molecular formula of the compound?

7. Given the balanced equation:

2Al + 3H₂SO₄ –> Al₂(SO₄)₃ + 3H₂

How many grams of H₂ are formed from 0.234 g of H₂SO₄?

8. Given the following balanced equation:

2KBr + Cl₂ –> 2KCl + Br₂

When 0.855 g of Cl₂ and 3.205 g of KBr react,

a. Determine the limiting reactant.

b. How many grams of Br₂ are formed?

c. How many grams of the excess reactant are needed for the reaction?

d. How many grams of the excess reactant will remain at the end of the reaction?

e. If 1.67 g of Br₂ are made in the reaction, what is the percent yield of Br₂?
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Chapter 4:

1. Calculate the molarity of a solution prepared by dissolving 1.37 g of Co(NO₃)₂ to make 24.9 mL of solution.

2. Assign oxidation numbers to all atoms in the following:

a. HNO₃ b. Cr₂O₇^2-

3. Given Ag + PtCl₂ –> AgCl + Pt

a. What is reduced?

b. What is oxidized?

c. What is the reducing agent?

d. What is the oxidizing agent?

4. How many grams of MgBr₂ are required to prepare a 250. mL solution with a concentration of 2.16 M?

5. 2Na₃PO₄ + 3Pb(NO₃)₂ –> 6NaNO₃ + Pb₃(PO₄)₂

What volume (mL) of a 0.100 M Na₃PO₄ is required to react with 150.0 mL of a 0.250 M Pb(NO₃)₂ solution?

6. Given BaCl₂(aq) + Na₂SO₄(aq) –>

a. Write the molecular equation.

b. Write the total ionic equation.

c. Write the net-ionic equation.

d. Identify the spectator ion(s).