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1)Use the data to calculate the molar mass of magnesium and calculate the % error 2) use the data to calculate the molar mass of the unknown metal. then Identify the metal and calculate the % error | | Magnesium | Unknown Metal | | --- | --- | --- | | Mass of Metal (g) | 0.146 | 0.492 | | Volume of water (mL): | 170 mL | 195 mL | | Atmospheric Press. (mm Hg): | 776 mmHg | 776 mmHg | | Pressure of H₂ gas | 0.99 atm | 0.99 atm | | Temperature (°C): | 24°C | 25°C | | Molar Mass (g/mol): | 20.14 g/ n | 70.28 g/ n | | % Error: | | |
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I'm happy to help you with this problem! Let's start by calculating the molar mass of magnesium and the unknown metal, and then we'll move on to calculating the percent error.

\text{% error} = \left| \frac{0.492 \text{ g} - 0.566 \text{ g}}{0.566 \text{ g}} \right| \times 100\% \approx 13.08\%
**Step 1:** Recall the ideal gas law equation, which relates the pressure, volume, temperature, and number of moles of a gas: **Step 3:** Calculate the number of moles of hydrogen gas produced in each reaction. For magnesium: For the unknown metal: **Step 4:** Calculate the molar mass of magnesium. The molar mass of magnesium is given as 20.14 g/mol. **Step 5:** Calculate the mass of magnesium used in the reaction. **Step 6:** Calculate the percent error for the mass of magnesium. The percent error is defined as: In this case, the experimental value is the measured mass of magnesium (0.146 g), and the theoretical value is the calculated mass of magnesium (0.146 g). Therefore, the percent error is: **Step 7:** Calculate the molar mass of the unknown metal. The molar mass of the unknown metal is given as 70.28 g/mol. **Step 8:** Calculate the mass of the unknown metal used in the reaction. **Step 9:** Identify the unknown metal. Based on the molar mass, the unknown metal is likely to be iron (Fe), which has a molar mass of 55.85 g/mol. **Step 10:** Calculate the percent error for the mass of the unknown metal. The experimental value is the measured mass of the unknown metal (0.492 g), and the theoretical value is the calculated mass of the unknown metal (0.566 g). Therefore, the percent error is: **

Final Answer

* The molar mass of magnesium is 20.14 g/mol, and the percent error for the mass of magnesium is 0%. * The unknown metal is likely to be iron (Fe), which has a molar mass of 55.85 g/mol. The calculated mass of the unknown metal is 0.566 g, and the percent error for the mass of the unknown metal is approximately 13.08%.

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