R= l*atm/mol*KPercent error= % ### Experiment Data and Calculations#### Overview:This experiment involves reacting magnesium metal with hydrochloric acid to produce hydrogen gas. The amount of hydrogen gas collected is then used to calculate the gas constant \( R \) and assess the percentage error compared to the ideal gas constant from the literature.#### Data Collected:- **Mass of Magnesium Metal**: 0.0422 g- **Volume of Collected Gas**: 43.9 mL- **Atmospheric Pressure**: 832 mmHg- **Temperature During Collection**: 32.0°C#### Water Vapor Pressure Table:This table provides the water vapor pressure at various temperatures, which is essential for correcting the pressure of the collected gas.| Temperature (°C) | Water Vapor Pressure (mmHg) ||------------------|------------------------------|| 26 | 25.2 || 28 | 28.3 || 30 | 31.8 || 32 | 35.7 || 34 | 39.9 || 36 | 44.6 |#### Calculations:- **Gas Constant (R):** Calculating this using the formula derived from the ideal gas law. \[ R = \frac{\text{L} \cdot \text{atm}}{\text{mol} \cdot \text{K}} \]- **Percent Error:** The deviation of the experimentally determined \( R \) from the literature value. \[ \text{Percent error} = 5.8\% \]#### Literature Value:The ideal gas constant from literature is provided as:- **\( R = 0.08206 \frac{\text{L} \cdot \text{atm}}{\text{mol} \cdot \text{K}} \)**This experiment is critical for understanding how real-life conditions affect the measurement of gas constants and assessing experimental accuracy through the percent error calculation.

The balanced reaction of Mg with HCl is as follows: Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g) Calculation of…

A student weighs out 0.0422 g of magnesium metal. The magnesium metal is reacted with excess hydrochloric acid to produce hydrogen gas. A sample of hydrogen gas is collected over water in a eudiometer at 32.0°C. The volume of Temperature °C Water Vapor Pressure (mmHg) 26 25.2 collected gas is 43.9 mL and the atmospheric pressure is 832 mmHg. Using the experimentally collected data, calculate R and the percent error. 28 28.3 30 31.8 32 35.7 34 39.9 36 44.6 Ideal gas constant from literature: L'atm R= mol·K L'atm 0.08206 mol·K Percent error=|5.8

A student weighs out 0.0422 g of magnesium metal. The magnesium metal is reacted with excess hydrochloric acid to produce hydrogen gas. A sample of hydrogen gas is collected over water in a eudiometer at 32.0°C. The volume of Temperature °C Water Vapor Pressure (mmHg) 26 25.2 collected gas is 43.9 mL and the atmospheric pressure is 832 mmHg. Using the experimentally collected data, calculate R and the percent error. 28 28.3 30 31.8 32 35.7 34 39.9 36 44.6 Ideal gas constant from literature: L'atm R= mol·K L'atm 0.08206 mol·K Percent error=|5.8

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

R= l*atm/mol*K

Percent error= %

### Experiment Data and Calculations

#### Overview:
This experiment involves reacting magnesium metal with hydrochloric acid to produce hydrogen gas. The amount of hydrogen gas collected is then used to calculate the gas constant \( R \) and assess the percentage error compared to the ideal gas constant from the literature.

#### Data Collected:
- **Mass of Magnesium Metal**: 0.0422 g
- **Volume of Collected Gas**: 43.9 mL
- **Atmospheric Pressure**: 832 mmHg
- **Temperature During Collection**: 32.0°C

#### Water Vapor Pressure Table:
This table provides the water vapor pressure at various temperatures, which is essential for correcting the pressure of the collected gas.

| Temperature (°C) | Water Vapor Pressure (mmHg) |
|------------------|------------------------------|
| 26 | 25.2 |
| 28 | 28.3 |
| 30 | 31.8 |
| 32 | 35.7 |
| 34 | 39.9 |
| 36 | 44.6 |

#### Calculations:
- **Gas Constant (R):** Calculating this using the formula derived from the ideal gas law.

\[
R = \frac{\text{L} \cdot \text{atm}}{\text{mol} \cdot \text{K}}
\]

- **Percent Error:** The deviation of the experimentally determined \( R \) from the literature value.

\[
\text{Percent error} = 5.8\%
\]

#### Literature Value:
The ideal gas constant from literature is provided as:
- **\( R = 0.08206 \frac{\text{L} \cdot \text{atm}}{\text{mol} \cdot \text{K}} \)**

This experiment is critical for understanding how real-life conditions affect the measurement of gas constants and assessing experimental accuracy through the percent error calculation.

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A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.
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