**Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas** according to the following equation:\[ 2\text{Al}(s) + 2\text{NaOH}(aq) + 6\text{H}_2\text{O}(l) \rightarrow 2\text{NaAl(OH)}_4(aq) + 3\text{H}_2(g) \]The product gas, \( \text{H}_2 \), is collected over water at a temperature of 20 °C and a pressure of 741 mm Hg. If the wet \( \text{H}_2 \) gas formed occupies a volume of 6.38 L, the number of moles of Al reacted was \(\underline{\hspace{2cm}}\) mol. The vapor pressure of water is 17.5 mm Hg at 20 °C. **Title: Preparation of Oxygen Gas by Heating Potassium Chlorate****Introduction:**Oxygen gas can be generated by heating potassium chlorate. The decomposition reaction is as follows:\[ 2 \text{KClO}_3(s) \rightarrow 2 \text{KCl}(s) + 3 \text{O}_2(g) \]**Experimental Details:**The product gas, \(\text{O}_2\), is collected over water at a temperature of 20 °C and a pressure of 751 mm Hg. If the wet \(\text{O}_2\) gas formed occupies a volume of 9.94 L, the task is to calculate the number of grams of \(\text{O}_2\) produced. The vapor pressure of water at 20 °C is 17.5 mm Hg.**Calculations:**1. **Correct the Pressure for Water Vapor:** Since the gas is collected over water, the pressure of the gas includes the pressure of the water vapor. To find the pressure of the dry \(\text{O}_2\), subtract the vapor pressure of water from the total pressure: \[ \text{P}_{\text{O}_2} = 751 \, \text{mm Hg} - 17.5 \, \text{mm Hg} \]2. **Use the Ideal Gas Law:** Apply the ideal gas law to find the moles of \(\text{O}_2\): \[ \text{PV} = \text{nRT} \] Where: - \( \text{P} \) is the corrected pressure in atm - \( \text{V} \) is the volume (9.94 L) - \( \text{n} \) is the number of moles - \( \text{R} \) is the ideal gas constant \((0.0821 \, \text{L} \cdot \text{atm/mol} \cdot \text{K})\) - \( \text{T} \) is the temperature in Kelvin3. **Convert Moles to Grams:** Use the molar mass of \(\text{O}_2\) (32.00 g/mol) to convert moles to grams.**Note:**Carry

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Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2AI9) + 2NaOH(aq) + 6H,00)—2NaA{ОН), (aq) + 3H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 741 mm Hg. If the wet H2 gas formed occupies a volume of 6.38 L, the number of moles of Al reacted was | |mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.

Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2AI9) + 2NaOH(aq) + 6H,00)—2NaA{ОН), (aq) + 3H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 741 mm Hg. If the wet H2 gas formed occupies a volume of 6.38 L, the number of moles of Al reacted was | |mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.

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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