Sodium metal reacts with water to produce hydrogen gas according to the following equation: 2Na(s) + 2H20(1)2NAOH(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 744 mm Hg. If the wet H2 gas formed occupies a volume of 9.27 L, the number of moles of Na reacted was mol. The vapor pressure of water is 17.5 mm Hg at 20 °C. Submit Answer Try Another Version 9 item attempts remaining

Sodium metal reacts with water to produce hydrogen gas according to the following equation: 2Na(s) + 2H20(1)2NAOH(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 20 °C and a pressure of 744 mm Hg. If the wet H2 gas formed occupies a volume of 9.27 L, the number of moles of Na reacted was mol. The vapor pressure of water is 17.5 mm Hg at 20 °C. Submit Answer Try Another Version 9 item attempts remaining

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

A 0.470 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H2SO4 (aq) →MSO4 (aq) + H2(g) A volume of 217 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 \deg C. The vapor pressure of water at 25 \deg C is 23.8 Torr. Calculate the molar mass of the metal.
At 61.1oC and 1.73 atm, 2.76 g of a hydrocarbon vapor has a volume of 1.62 L. What is the molecular weight in g/mol of the hydrocarbon?
A 0.483 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 209 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
How many liters of sulfur dioxide gas can be produced at STP by the addition of 9.62 mol of hydrochloric acid (HCl) to sodium sulfite if sodium chloride and water are also produced?
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.
How many liters of sulfur dioxide gas can be produced at STP by the addition of 9.98 mol of hydrochloric acid (HCl) to sodium sulfite if sodium chloride and water are also produced?
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 550. L and heated to 520.0 °C. When the amount of CaCO3 has stopped changing, it is found that 8.46 kg have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 520.0 °C. Round your answer to 2 significant digits. P Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. 0 X
lithium reacts with H2O to produce hydrogen.(a) Write a balanced chemical equation for the reaction, using the smallest integer coefficients possible. Write states in brackets. (Hint: LiOH is the second product.) (b) Calculate the mass of pure Li that will furnish 16.3 L of hydrogen at a pressure of 0.860 atm and a temperature of 30.4°C.
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete the lime absorbs CO₂ from the air and turns back into hard, durable 2 limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 400. L and heated to 740.0 °C. When the amount of CaCO3 has stopped changing, it is found that 3.37 kg have disappeared. P 00. Calculate the pressure equilibrium constant K this experiment suggests for the equilibrium between CaCO3 and CaO at 740.0 °C. Round your answer to 2 significant digits. Ar Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. р K₁ = 0 x10 р x Ś ? Explanation Check 0 81 K © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility