Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation:2Al(s) + 2NAOH(aq) + 6H2O(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 752 mm Hg. If the wet H2 gas formed occupies a volume of 6.17L, the number of moles of Al reacted wasmol. The vapor pressure of water is 23.8 mm Hg at 25 °C.

Answered: Image /qna-images/answer/ffa2354d-a254-4b54-9e2b-0d22fb24448e.jpg

Al(s) + 2NaOH(aq) + 6H2O(1)2NAAI(OH)4(aq) + 3H2(g) he product gas, H,, is collected over water at a temperature of 25 °C and a pressure of 752 mm Hg. If the wet H, gas formed occupies a volume of 6.17 the number of moles of Al reacted was mol. The vapor pressure of water is 23.8 mm Hg at 25 °C.

Al(s) + 2NaOH(aq) + 6H2O(1)2NAAI(OH)4(aq) + 3H2(g) he product gas, H,, is collected over water at a temperature of 25 °C and a pressure of 752 mm Hg. If the wet H, gas formed occupies a volume of 6.17 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

(c) A halothane-oxygen gas mixture is placed in an enclosed container. The partial pressure of halothane and oxygen are 170 kPa and C, respectively. The mole fraction of oxygen gas is 0.458. (i) Calculate the total pressure of halothane-oxygen mixture. (ii) Determine the partial pressure of oxygen, C.
EXERSICE 7 (A) Let A and B be two ideal gases at the same temperature. If mÃ>m³ (where mÃ, m³ are the masses of molecules of gases A and B, respectively) and EA, E, the average kinetic energies of the two gases, choose the correct phrase, giving a justification. (1) EA = EB (ii) EA > EB (iii) EA < EB (iv) Data are insufficient to compare EA, EB.
A gas mixture contains 4.5 mol Br, and 33.1 mol F,. (a) Compute the mole fraction of Br, in the mixture. (b) The mixture is heated above 150°C and starts to react to give BrFs: Br2(g) + 5 F2(g) –→ 2 BrF;(g) At a certain point in the reaction, 2.2 mol BrF5 is present. Determine the mole fraction of Br2 in the mixture at that point.
Given 2Na(s) + 2H2O(l) --> 2NaOH(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 20°C and a pressure of 759 mm Hg. If the wet H2 gas formed occupies a volume of 7.42L, how many grams of H2 are formed? The vapor pressure of water is 17.5 mm Hg at 20°C.
1) a) Sulfuric acid, the industrial chemical produced in the greatest quantity each year, is prepared by the reaction of sulfur in the presence of oxygen and water as described in the balanced chemical equation below. Calculate the volume, in ml, of 18.0 M sulfuric acid solution that can be prepared from the reaction of 1850 g of sulfur with 6.50E4ML oxygen gas at 25°C and 0.965atm and plenty of water. 25(solid) + 302 (gas) + 2H20(liquid) > 2H:SO4(aqueous) b. Which substance is the limiting reactant? Explain how you know.
A 0.516 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) MSO,(aq) + H,(g) A volume of 223 ml. of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 "C. The vapor pressure of water at 25 "C is 23.8 Torr. Calculate the molar mass of the metal. g/mol molar mass:
A sample of hydrogen (H2) gas was collected over water at 60°C. If the total volume of gas collected was 71.8 mL and the atmospheric pressure was 1.02 bar, what mass (in g) of hydrogen gas was collected above the water? The vapour pressure of water at 60°C is 150 torr.
in the following reaction, 27.1 mL of o2(g) is collected over water at 23*C and barometric pressure 751 mmHg. After the reaction, the buret could not be lowered far enough to make the water levels equal in both the burette and beaker. In fact, you measured the difference in water levels to be 34 mm, what must have been the mass of the Ag2O decomposed? (the vapor pressure of water at 23* C is 21.1 mmHg)
1) a) Sulfuric acid, the industrial chemical produced in the greatest quantity each year, is prepared by the reaction of sulfur in the presence of oxygen and water as described in the balanced chemical equation below. Calculate the volume, in ml, of 18.0 M sulfuric acid solution that can be prepared from the reaction of 1850 g of sulfur with 6.50x10'mL oxygen gas at 25°C and 0.965atm and plenty of water. 25(solid) + 302 (gas) + 2H20(liquid) _-→ 2H2SO4(aqueous) b. Which substance is the limiting reactant? Explain how you know.
A 0.265 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H,SO,(aq) → MSO,(aq) + H,(g) A volume of 277 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr, and the temperature is 25 °C. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal. molar mass: g/mol
(a) (c) A column of water in a buret is 336 mm Hg high. How high would that column be if it were mercury instead of water? (d) In order for the pressures to be equal, density and height of a column are inversely proportional, therefore the following relationship applies: (denHg)(hHg) = (denH20)(hH20) Note: the density of mercury is 13.6 g/mL and the density of water is 1.00 g/mL. An electrolysis experiment was run for 15 minutes and 45 seconds at an average current of 189 milliamps (mA). The mass lost by the copper anode was 0.0589 grams. (b) Calculate the number of coulombs transferred. (Remember: coulomb = amps x sec) Show full calculation of the height in mercury (remember to use proper significant figures.) Calculate the moles of copper lost from the anode. Based on the moles of copper lost determined in 1c, calculate the moles of electrons transferred. Remember, the reaction at the copper anode is: Cu(s)---> Cu¹² (aq) + 2 e
In order to produce solid iron, it first must bc processed from its orc, Fe2O1, in a blast furnace. During operation, CO gas (flue gas) is introduced into the furnace at 1650 °C and a pressure of 250 kPa. In this process flue gas reduces iron to its elemental form in the following reaction: 41. Fe;O30) COg Fe+ COz At one point in this process 256.0 L of CO was used to reduce iron ore. Assuming a complete reaction, how many grams of solid iron can be produced. Balanced chemical equation: Mass of Fe (in grams)