**Chemical Reaction of Aluminum with Sodium Hydroxide to Produce Hydrogen Gas**Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation:\[ 2\text{Al(s)} + 2\text{NaOH(aq)} + 6\text{H}_2\text{O(l)} \rightarrow 2\text{NaAl(OH)}_4\text{(aq)} + 3\text{H}_2\text{(g)} \]In this reaction, the product gas, \(\text{H}_2\), is collected over water at a temperature of 25°C and a pressure of 744 mm Hg. If the wet \(\text{H}_2\) gas formed occupies a volume of 6.55 L, the number of moles of Al reacted was ____ mol. The vapor pressure of water is 23.8 mm Hg at 25°C.**Explanation:**- **Reaction Description**: Aluminum (Al) reacts with sodium hydroxide (NaOH) and water (H₂O) to produce sodium aluminate (\(\text{NaAl(OH)}_4\)) in aqueous solution and hydrogen gas (\(\text{H}_2\)).- **Conditions**: The reaction conditions include a temperature of 25°C and a pressure of 744 mm Hg. The vapor pressure of water at this temperature is 23.8 mm Hg.- **Objective**: Calculate the number of moles of aluminum that reacted, given that the volume of the gas collected is 6.55 L.Graphs or diagrams were not present in the image.

Given, Pressure of H2 gas= 744 mm of Hg = 744760atm T= 25°C= 298K…

Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2Al(s) + 2NAOH(aq) + 6H20(1)-2NAAI(OH)4(aq) + 3H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 744 mm Hg. If the wet H, gas formed occupies a volume of 6.55 L, the number of moles of Al reacted was mol. The vapor pressure of water is 23.8 mm Hg at 25 °C.

Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2Al(s) + 2NAOH(aq) + 6H20(1)-2NAAI(OH)4(aq) + 3H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 744 mm Hg. If the wet H, gas formed occupies a volume of 6.55 L, the number of moles of Al reacted was mol. The vapor pressure of water is 23.8 mm Hg at 25 °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...

See similar textbooks

Similar questions

What volume of hydrogen gas (in mL) at 707 mm Hg and 42 °C can be produced when 2.1 g of CaCO3(s) are put into an Erlenmeyer flask containing 225 mL of 0.261 M HCl(aq) ?1 CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)
1.) This reaction occurs in large test tube at 32.0oC: 2 Al (s) + 3 H2SO4(aq) ---> 6 H2 (g) + Al2(SO4)3 (aq) A tube going through the stopper of the test tube feeds into a graduated cylinder that has been inverted in a tub of water. At the end of the reaction, the total pressure of gas in the inverted cylinder is 435. torr, and the volume of gas collected is 455. mL. What mass of aluminum must have reacted? P.s- please show how you got it. I get confused with it
+7 (A) 15.2 L B) 0 C) +3 D) -2 19. 68.1 g solid CaCO3 is mixed with excess HC1. What is the volume of CO2 will be collected at 0.0 °C, and 1 atm. (Molar mass CaCO3 = 100.08 g/mol, CO₂ = 44.1 g/mol CaCO3 (s) + 2 HCl(aq) → H₂O (1) +CaCl2 (aq) + CO₂(g) C) OL B) 29.9 L C D) 155 L 20. A gas sample has an initial volume of 0.500 L and initial pressure of 1.0 atm. Wha the volume when the pressure of the sample is decreased to 0.50 atm? Assume the temperature and number of moles of the gas are constant. P₁V₁ = P₂1 A) .0 L B) 0.025 L
Use the ideal gas equation, PV = nRT, to calculate the pressure in torr of 1.823 moles of oxygen gas collected at 27.9°C with a volume of 40.52 liters. The gas was not collected over water. R = 82.1 atm·mL/mol·K or R = 0.0821 atm·L/mol·K
Consider the reaction of a mixture of NaHCO3 and Ca(HCO3)2 with excess HCl. The net ionic reaction observed is H+(aq) + HCO3-(aq) → H2O(l) + CO2(g) The above sample of gas (15.2 L, STP) contains 0.447 mol of N2. What is the mole fraction of nitrogen in that sample of gas? X = ___
When aluminum is placed in concentrated hydrochloric acid, hydrogen gas is produced. 2 Al(s) + 6 HCI(aq) →2 AICI, (aq) + 3 H, (g) What volume of H, (g) is produced when 7.30 g Al(s) reacts at STP? volume of H, (g): L.
Calcium carbide reacts with water to produce acetylene gas according to the following equation: CaC₂ (s) + 2H₂O(1)→ C₂H₂(g) + Ca(OH)2 (aq) The product gas, C₂ H2, is collected over water at a temperature of 20 °C and a pressure of 742.0 mm Hg. If the wet C₂2H2 gas formed occupies a volume of 9.02 L, the number of moles of CaC2 reacted was mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.
12b
What volume of H2 gas, measured at 9 °C and 722 torr, can be obtained by reacting 8.40 g of zinc metal with 185 mL of 0.425 M HCl? (6 marks) Zn(s) + 2 HCl (aq) → ZnCl2(aq) + H2(g) (1 atm = 760 torr)
37. What volume of H, gas, measured at 27°C and 700. torr, can be obtained by reacting 5.00 g of zinc metal with 100. mL of 0.350 M HCI? The equation is Zn(s) + 2 HCl(aq) – → ZnCl(ag) + H2(g)
How many grams of AL were reacted with excess HCI if 4.78L of hydrogen gas were collected at STP in the following reaction? 2 AL (s) + 6 HCI (aq) = 2 AICI3 (aq) + 3 H2 (g)
Hydrogen gas is produced by the reaction between metallic aluminum and aqueous hydrochloric acid. 2 Al(s) + 6HCl(aq) 2 AlCl3(aq) + 3 H₂(g) The hydrogen gas produced by this reaction is typically collected via water displacement. During this process, the hydrogen gas becomes saturated with water vapor. If 280.5 mL of gas with a total pressure of 1.14 atm is collected via water displacement at 29.4 °C, what is the partial pressure of the hydrogen gas in the sample? The vapor pressure of water at 29.4 °C is 30.75 torr. atm PH₂ = How many grams of aluminum must have reacted to produce this quantity of hydrogen gas? mass of aluminum: