Some commercial drain cleaners use a mixture of sodium hydroxide and aluminum powder. When the solid mixture is poured into the drain and dissolves, a reaction ensues that produces hydrogen gas: 2NAOH(aq) + 2AI(s) + 6H20() → 2NAAI(OH)4(aq) + 3H2(g) Determine the volume (in L) of hydrogen gas produced when 18.77 g of aluminum reacts with excess sodium hydroxide and water if the temperature is 29.59 °C and the pressure is 106.79 kPa. Provide your answer with TWO decimals. Your Answer:

Some commercial drain cleaners use a mixture of sodium hydroxide and aluminum powder. When the solid mixture is poured into the drain and dissolves, a reaction ensues that produces hydrogen gas: 2NAOH(aq) + 2AI(s) + 6H20() → 2NAAI(OH)4(aq) + 3H2(g) Determine the volume (in L) of hydrogen gas produced when 18.77 g of aluminum reacts with excess sodium hydroxide and water if the temperature is 29.59 °C and the pressure is 106.79 kPa. Provide your answer with TWO decimals. Your Answer:

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 3CR

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Nitrous oxide (N₂O), also known as laughing gas, has uses in surgery and dentistry as an anesthetic. The molecular weight of the nitrous oxide cylinder is 44.013 g/mol. Assuming standard temperature and pressure, what would be the volume, in L, of a cylinder containing 4.23 kg of nitrous oxide?
On January 28, 2014, in Germany, a barn containing 90 cows exploded when a stray spark caught the methane trapped in the building on fire. The building was damaged and one cow was slightly injured with minor burns. Assume that the 90 cows were producing 250L of methane per day and that there was a 15 hour collection in the barn when it ignited. __CH4 + __O2 → __ CO2 + __H2O a) How many liters of methane was in the barn when it exploded? b) What mass of water was generated in the explosion? (SET WORK INTO TRAIN TRACKS)
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Consider the following data gathered in the "Molar Mass of a Gas" experiment. * Mass of the empty reaction test tube: _____27.54_____ g * Mass of the test tube and MnO2 used in the reaction: ____28.04___ g * Mass of the test tube, KClO3 (MM = 122.55 g/mol) and MnO2 used in the reaction: ____29.31___ g * Mass of the test tube and its contents after the reaction: ____ (2.87x10^1) _____ g * Volume of the bubble of oxygen generated in the experiment: ___356___ mL * Atmospheric pressure in the lab: ______766.06______ mm Hg * Vapor pressure at reaction temperature: _____18.6_____ m Hg Calculate the mass of oxygen generated in the reaction
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Phosphoric acid and magnesium hydroxide react to produce magnesium phosphate and water. If 45.00 mL of 1.50 M phosphoric acid are used in the reaction, how many grams of magnesium hydroxide are needed for the reaction to go to completion?
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