The moles of hydrogen which are produced from 57.5 grams of lithium is 8.21 grams.
<h3>What is stoichiometry?</h3>
Stoichiometry of the reaction gives idea about the relative amount of product produced by the reactant in terms of moles.
Given chemical reaction is:
2Li(s) + H₂O(l) → 2LiOH(aq) + H₂(g)
Moles of lithium will be calculated as:
n = W/M, where
- W = given mass = 57.5g
- M = molar mass = 7g/mol
n = 57.5 / 7 = 8.21 mol
From the stoichiometry of the reaction:
- 2 moles of Li = produces 1 mole of H₂
- 8.21 moles of Li = produces 8.21/2=4.105 moles of H₂
Mass of H₂ = (4.105mol)(2g/mol) = 8.21g
Hence required mass of hydrogen gas is 8.21g.
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The addition of an electron on to the element of hydrogen and ultimately to the electron carrier is an example of reduction. The molecule is becoming reduced or has electrons, and or hydrogen to help facilitate the addition of the electrons on it.
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Answer:
72.71 %
Explanation:
CO2. % C = 12.01/44.01 = 0.2729= 27.29% (we will divide 0.2729 with 100 to take the percentage). % O = 32.00/44.01 =0.7271 =72.71 %O in CO2.
