What volume of hydrogen gas is produced when 93.6 g of iron reacts completely according to the following reaction at 25 °C and 1 atm? iron(s) + hydrochloric acid (aq) → iron(II) chloride (aq) + hydrogen (g) L Volume =

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**Hydrogen Gas Production**

To determine the volume of hydrogen gas produced when 93.6 grams of iron reacts completely, we refer to the following chemical reaction:

\[ \text{iron}(s) + \text{hydrochloric acid}(aq) \rightarrow \text{iron(II) chloride}(aq) + \text{hydrogen}(g) \]

Assume the reaction occurs at 25°C and 1 atm.

The aim is to calculate the volume of hydrogen gas produced. 

\[ \text{Volume} = \_\_\_\_ \text{L} \]

Make use of stoichiometry, molar mass, and the ideal gas law to solve the problem.
Transcribed Image Text:**Hydrogen Gas Production** To determine the volume of hydrogen gas produced when 93.6 grams of iron reacts completely, we refer to the following chemical reaction: \[ \text{iron}(s) + \text{hydrochloric acid}(aq) \rightarrow \text{iron(II) chloride}(aq) + \text{hydrogen}(g) \] Assume the reaction occurs at 25°C and 1 atm. The aim is to calculate the volume of hydrogen gas produced. \[ \text{Volume} = \_\_\_\_ \text{L} \] Make use of stoichiometry, molar mass, and the ideal gas law to solve the problem.
### Solving the Equation

Multiply both sides of the equation by the same expression:

(Be sure that the answer field changes from light yellow to dark yellow before releasing your answer.)

\[ \times \left( [A] - [A]_0 \right) = \quad \times (-kt) \]

#### Instructions:
Drag and drop your selection from the following list to complete the answer:

|          |     |     | 
|----------|-----|-----|
| \(\frac{1}{k}\) | \(k\) | \(-k\) | \(- \frac{1}{k}\) |

To solve the provided equation, you need to drag and drop the correct expression into the blue blank spaces on each side of the equation.

#### Explanation:
- **Left side of the equation**: Multiply \([A] - [A]_0\) by your chosen expression.
- **Right side of the equation**: Multiply \(-kt\) by the same expression for balance.

### Graphs or Diagrams Explanation:
There are no graphs or diagrams present in this specific exercise.

Use the options provided to ensure both sides of the equation are balanced correctly.
Transcribed Image Text:### Solving the Equation Multiply both sides of the equation by the same expression: (Be sure that the answer field changes from light yellow to dark yellow before releasing your answer.) \[ \times \left( [A] - [A]_0 \right) = \quad \times (-kt) \] #### Instructions: Drag and drop your selection from the following list to complete the answer: | | | | |----------|-----|-----| | \(\frac{1}{k}\) | \(k\) | \(-k\) | \(- \frac{1}{k}\) | To solve the provided equation, you need to drag and drop the correct expression into the blue blank spaces on each side of the equation. #### Explanation: - **Left side of the equation**: Multiply \([A] - [A]_0\) by your chosen expression. - **Right side of the equation**: Multiply \(-kt\) by the same expression for balance. ### Graphs or Diagrams Explanation: There are no graphs or diagrams present in this specific exercise. Use the options provided to ensure both sides of the equation are balanced correctly.
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