1. When the following equation is balanced, what is the coefficient for H₂O? Ca(OH)₂(aq) + H₃PO₄(aq) → Ca₃(PO₄)₂(s) + H₂O(l)
(A)2
(B)3
(C)4
(D)6

2. A substance that, when dissolved in water, produces a solution that conducts electric current very efficiently is called (A) a strong electrolyte (B) a weak electrolyte (C) a strong ion (D) an electrical solute

3. Classify the reaction : \[ \text{Cu(NO}_3)_2\text{(}\textit{aq}\text{)} + 2\text{NaOH(}\textit{aq}\text{)} \rightarrow \text{Cu(OH)}_2\text{(s)} + 2\text{NaNO}_3\text{(}\textit{aq}\text{)} \] (A) formation of a solid (B) formation of a gas (C) formation of water (D) transfer of electrons

4. The equation 2C2H6 + 7O2 → 4CO2 + 6H2O is an oxidation-reduction reaction. Which statement is true? (A) the carbon is reduced, and the oxygen is oxidized (B) the carbon is oxidized, and the hydrogen is reduced (C) the carbon is oxidized, and the oxygen is reduced (D) it is a decomposition reaction

5. \( \text{Cu(NO}_3)_2\text{(aq)} + 2\text{NaOH(aq)} \rightarrow \text{Cu(OH)}_2\text{(s)} + 2\text{NaNO}_3\text{(aq)} \)Which one is the net ionic equation?(A) \( \text{Cu}^{2+}\text{(aq)} + 2\text{NO}_3^-\text{(aq)} \rightarrow \text{Cu(NO}_3)_2\text{(aq)} \)(B) \( \text{Cu}^{2+}\text{(aq)} + 2\text{OH}^-\text{(aq)} \rightarrow \text{Cu(OH)}_2\text{(s)} \)(C) \( 2\text{NO}_3^-\text{(aq)} + 2\text{Na}^+\text{(aq)} \rightarrow 2\text{NaNO}_3\text{(aq)} \)(D) \( \text{Na}^+\text{(aq)} + \text{OH}^-\text{(aq)} \rightarrow \text{NaOH(s)} \)

6. How many electrons are transferred in the following redox reaction?  Zn(s) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s) (A)1 (B)2 (C)3 (D)4

7. Finish and balance the neutralization reaction: HClO4 (aq) + Ba(OH)2 (aq) → (A) H2O (l) + BaCl2 (aq) (B) H2O (l) + Ba(ClO4)2 (s) (C) H2O (l) + Ba(ClO4)2 (aq) (D) BaO (s) + Cl2 (g) + H2O (l)

8. Al(s) + I2(g) → AlI3(s). Which one is correct? (A) I2 is oxidized (B) Al is reduced (C) Al is a reducing agent (D) I2 is a reducing agent

9. Calculate the molar mass of a sample with a single molecule weighs \(9.31 \times 10^{-23}\) g.(A) 56.1 g/mol(B) \(6.47 \times 10^{45}\) g/mol(C) \(6.02 \times 10^{23}\) g/mol(D) \(9.31 \times 10^{-23}\) g/mol

10. What percentage of nitrogen contained in (NH4)2CO3 by mass? (A) 58.3% (B) 14.6% (C) 29.2% (D) 18.8% 

11. The molar mass of a compound is 100 g/mol with the percent composition (by mass) of C : H : O = 65.45% : 5.45% : 29.09%. Determine the empirical formula and the molecular formula. (A) CHO and C6H6O6 (B) C3H3O and C6H6O2 (C) C3HO and C6H2O2 (D) CH2O and C4H8O4

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