QuestionMarch 21, 2026

Part 1: In the space below, use the periodic table and show how to calculate the molar mass of water (H_(2)O) and oxygen gas (O_(2)) Molar mass of H2O: H_(2)O:underline ( )g/mol Part 2: Balance and classify the reaction for the creation of oxygen gas (O_(2)) from water (H_(2)O) Fill in the blanks to balance the chemical reaction below: What type of reaction is this? (circle the correct answer) a. Single Replacement b. Double Replacement c. Combustion d. Decomposition underline ( )H_(2)O(l)arrow underline ( )H_(2)(g)+underline ( )O_(2)(g) Molar mass O_(2):underline ( )g/mol

Part 1: In the space below, use the periodic table and show how to calculate the molar mass of water (H_(2)O) and oxygen gas (O_(2)) Molar mass of H2O: H_(2)O:underline ( )g/mol Part 2: Balance and classify the reaction for the creation of oxygen gas (O_(2)) from water (H_(2)O) Fill in the blanks to balance the chemical reaction below: What type of reaction is this? (circle the correct answer) a. Single Replacement b. Double Replacement c. Combustion d. Decomposition underline ( )H_(2)O(l)arrow underline ( )H_(2)(g)+underline ( )O_(2)(g) Molar mass O_(2):underline ( )g/mol
Part 1: In the space below, use the periodic table and show how to calculate the molar mass of water (H_(2)O) and oxygen gas (O_(2)) Molar mass of H2O: H_(2)O:underline ( )g/mol Part 2: Balance and classify the reaction for the creation of oxygen gas (O_(2)) from water (H_(2)O) Fill in the blanks to balance the chemical reaction below: What type of reaction is this? (circle the correct answer) a. Single Replacement b. Double Replacement c. Combustion d. Decomposition underline ( )H_(2)O(l)arrow underline ( )H_(2)(g)+underline ( )O_(2)(g) Molar mass O_(2):underline ( )g/mol

Solution
4.4(264 votes)

Answer

Molar mass H_2O: 18.016 g/mol ### Molar mass O_2: 32.00 g/mol ### Balanced reaction: 2H_2O(l) \rightarrow 2H_2(g) + O_2(g) ### Reaction type: Decomposition Explanation 1. Calculate molar mass of H_2O Atomic mass of H: 1.008 g/mol, O: 16.00 g/mol. **Molar mass formula:** M = \sum (\text{atomic mass} \times \text{subscript}) M_{H_2O} = (2 \times 1.008) + (1 \times 16.00) = 2.016 + 16.00 = 18.016 g/mol. 2. Calculate molar mass of O_2 M_{O_2} = 2 \times 16.00 = 32.00 g/mol. 3. Balance the reaction Decomposition of water: Unbalanced: H_2O \rightarrow H_2 + O_2 Balanced: **2H_2O(l) \rightarrow 2H_2(g) + O_2(g)** 4. Classify reaction type Water breaking into simpler substances = Decomposition.

Explanation

1. Calculate molar mass of $H_2O$ <br /> Atomic mass of H: 1.008 g/mol, O: 16.00 g/mol. <br />**Molar mass formula:** $M = \sum (\text{atomic mass} \times \text{subscript})$ <br />$M_{H_2O} = (2 \times 1.008) + (1 \times 16.00) = 2.016 + 16.00 = 18.016$ g/mol. <br /><br />2. Calculate molar mass of $O_2$ <br /> $M_{O_2} = 2 \times 16.00 = 32.00$ g/mol. <br /><br />3. Balance the reaction <br /> Decomposition of water: <br />Unbalanced: $H_2O \rightarrow H_2 + O_2$ <br />Balanced: **$2H_2O(l) \rightarrow 2H_2(g) + O_2(g)$** <br /><br />4. Classify reaction type <br /> Water breaking into simpler substances = Decomposition.
Click to rate:

Similar Questions