![]() ![]() We can begin by noticing that the reactant side of the equation has two oxygen atoms and the product side only has one oxygen atom. And in this reaction, there is one product, water, which has the chemical formula H2O. The products are written on the right side of the reaction arrow. The reactants are always written on the left side of the reaction arrow in a chemical equation. The chemical formula for diatomic oxygen is O2, and the chemical formula for diatomic hydrogen is H2. Let’s start by writing the chemical formulas of the reactants. Because we are using stoichiometry to solve this problem, a balanced chemical equation is needed. The reactant that could produce less water is the limiting reactant and therefore determines the amount of water produced. In order to solve this problem and determine the mass of water formed in the reaction, we need to calculate the amount of water each reactant would produce if fully consumed. ![]() We need to find out if a limiting reactant is present, which would limit the amount of the product, water, being formed. In order to determine if the masses of both reactants are completely consumed, we need to rely on our knowledge of stoichiometry. So if 4.800 grams of oxygen and 0.5846 grams of hydrogen are completely consumed during a reaction, then we’d expect that 5.3846 grams of water should be produced. However, this assumes that all of the reactant molecules are completely consumed during the reaction. To begin, we may initially think about the law of conservation of mass, which states that in a closed system, the mass of reactants of a chemical reaction will equal the mass of the products. The molar mass of hydrogen is one gram per mole and oxygen is 16 grams per mole. ![]() How much water can be produced from 4.800 grams of oxygen and 0.5846 grams of hydrogen? Give your answer to the nearest two decimal places. ![]()
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