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Scan_Doc0012 - EXAMPLE 3.15:== Solid lithium hydroxide is...

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3.1.0 Stoichiometric CaLcuLations: Amounts of Reactants and Products 105 PROBLEM-SOLVING STRATEGY CaLcuLating Masses of Reactants and Products in ChemicaL Reactions 1 ~ Balance the equation for the reaction. 2 ~ Convert the known mass of the reactant or product to moles of that substance. 3 ~ Use the balanced equation to set up the appropriate mole ratios. 4 ~ Use the appropriate mole ratios to calculate the number of moles of the desired reactant or product. . 5 ~ Convert from moles back to grams if required by the problem. Balanced chemical equation Moles desired substance Moles known substance l Convert to moles I Moles of known substance Use mole ratio I· 1 Convert I to convert Moles of . to grams . Mass of I desired j • desired substance substance Mass of known substance
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Unformatted text preview: EXAMPLE 3.15--:== Solid lithium hydroxide is used in space vehicles to remove exhaled carbon dioxide from the living environment by forming solid lithium carbonate and liquid water. What mass of gaseous carbon dioxide can be absorbed by 1.00 kg of lithium hydroxide? SoLution Where are we going? • To find the mass of CO 2 absorbed by 1.00 kg LiOH What do we know? ./ Chemical reaction LiOH(s) + CO 2 (g)----* Li 2 C0 3 (s) + H 2 0(I) ./ 1.00 kg LiOH What information do we need to find the mass of CO 2 ? ./ Balanced equation for the reaction How do we get there? 1 ~ What is the balanced equation? 2LiOH(s) + CO 2 (g)---+ Li 2 C0 3 (s) + H 2 0(l)...
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