Concept explainers
Alkali metal hydroxides are sometimes used to “scrub” excess carbon dioxide from the air in closed spaces (such as submarines and spacecraft). For example, lithium hydroxide reacts with carbon dioxide according to the unbalanced chemical equation
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ppose a lithium hydroxide canister contains 155 g of
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Chapter 9 Solutions
Introductory Chemistry: A Foundation
- Copper reacts with nitric acid according to the following reaction. 3Cu(s)+8HNO3(aq)3Cu(NO3)2(aq)+2NO(g)+4H2O(l) If 2.40 g of Cu is added to a container with 2.00 mL of concentrated nitric acid (70% by mass HNO3; density = 1.42 g/cm3), what mass of nitrogen monoxide gas will be produced?arrow_forwardNapeleon doesn’t think the water is clean enough at the water park “Waterloo”. In an effort to sanitize the water, Napeleon (he has OCD) knows that bromine can be used to purify the water at the water park. If 7.82 x 1021 formula units of sodium bromide are reacted with excess chlorine gas, how many milliliters of liquid bromine (density = 3.12 g/mL) are formed? 2 NaBr (s) + Cl2 (g) à 2 NaCl (s) + Br2 (l) (BALANCED)arrow_forwardThe production of ammonia nia * (N*H_{3}) from nitrogen and hydrogen, shown below, was an important breakthrough resulting in Nobel prizes in chemistry to Fritz Haber (1918) and Carl Bosch (1931). This compound is widely used in manufacturing fertilizers. 3H 2 (g)+N 2 (g) 2NH 3 (g) Calculate the mass of nitrogen (in kg ) needed to manufacture 1000 kg of ammonia . Assume four significant figures .arrow_forward
- The great French chemist Antoine Lavoisier discovered the law of conservation of mass in part by doing a famous experiment in 1775. In this experiment they found that mercury(II) oxide, when heated, decompose into liquid mercury and an invisible and previously unknown substance: oxygen gas. A. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury (II) oxide (HgO) into liquid mercury and gaseous dioxygen. B. Suppose 72 mL of dioxygen gas are produced by this reaction, at a temperature of 120°C and pressure of exactly 1 atm. Calculate the mass of mercury (II) oxide that must have reacted in grams. Round your answer to three significant digits.arrow_forwardA side reaction in the manufacture of rayon from wood pulp is 3CS2+6NaOH→2Na2CS3+Na2CO3+3H2O How many grams of Na2CS3 are produced in the reaction of 92.5 mL of liquid CS2 (d = 1.26 g/mL) and 2.61 mol NaOH? Express your answer with the appropriate units.arrow_forward1 Sr + 2 H2O → 1 Sr(OH)2 + 1 H2 Given 9.24×10-1 g of H2O, determine the mass (in grams) of Sr that is required to completely react with all of the H2O. Please give the answer with three significant figures.arrow_forward
- Thermite welding is an exothermic reaction, which produces molten iron that permanently binds metals as it cools. The process does not require heat or electricity. Aluminum powder is simply mixed with ferric oxide powder. The reaction is accompanied by a release of heat, and produces aluminum oxide and molten iron. The equation shows: 2 Al + Fe2O3 = Al2O3 + 2 Fe If 55.0 grams of aluminum powder is mixed with 75.0 grams of ferric oxide, which of the two substances is the limiting reagent? The excess reagent? How many grams of molten iron (Fe) will be produced?arrow_forwardCommercial drain cleaners contain sodium hydroxide and aluminum. When water is added to this mixture, the heat that is generated will melt grease and the gas that is created will stir up the particles that are clogging the drain. If the process proceeds according to the following reaction: 2 Al (s) + 2 NaOH (aq) + 6 H2O (l) → 2 NaAl(OH)4 (aq) + 3 H2 (g) If you use 5.6 g of Al (s) and excess sodium hydroxide, how many liters of H2 (g) at 742 mm Hg and 22.0 ˚C are produced?arrow_forwardIf 30.2 mL of 6M HCl are involved in the Grignard reaction, how many moles of HCl are involved in the reaction? Round your answer to the correct number of significant figuresarrow_forward
- For this question, you will review the student’s work below and identify the errors they made in their calculations. A student wanted to make a huge volcano from vinegar and baking soda. If they used an entire box of baking soda (525 g), how much vinegar would they need? (most vinegar we buy at the store is 5%) NaHCO3(s)+HCH3COO(aq)—>H2O(l)+NaCH3COO(aq)+CO2 (g) They calculate the amount of vinegar using the following calculation. First, they decide to start with 1 mole of acetic acid and then multiply it by the mole ratio of 1:1 of acetic acid to baking soda. After that, they multiply by the grams of baking soda to end up with grams of acetic acid. 1) Provide at least two problems(provide specific examples)with their process and calculations. 2) Re-calculate the amount of vinegar needed to make a volcano using proper stoichiometryarrow_forwardOxygen masks, used for producing oxygen gas in emergency situations, react potassium superoxide (KO2) with water and carbon dioxide to produce potassium bicarbonate and oxygen gas according to the reaction shown. How many grams of potassium superoxide (KO2) should the mask have if each mask needs to produce 27.6 g of oxygen gas? Your answer should include the correct number of significant figures. Upload a picture or pdf of your work and answer. * 4KO2 + 2 H2O + 4 CO2 -----> 4KHCO3 + 3O2arrow_forwardSO2 is a product of coal combustion. It may combine with O2 and H2O in the atmosphere to form sulfuric acid, a component of acid rain. One way to reduce the formation of acid rain involves trapping the SO2 by passing smokestack gases through a spray of calcium oxide and O2. The product of this reaction is calcium sulfate. a) Write a balanced chemical equation describing this reaction by writing the product and adding coefficients. __SO2+__CaO+__O2=__CaSO4 b) How many metric tons of calcium sulfate would be produced from each metric ton of SO2 that is trapped?arrow_forward
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