Multiple Choice
Zinc metal reacts with aqueous silver nitrate to form solid silver and aqueous zinc nitrate. If 2.00 g of zinc react with 2.50 g of silver nitrate, how many grams of silver will form?
3. Chemical Reactions
Stoichiometry
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How many grams of oxygen (O2) are needed to completely react with 1.33 g of butyric acid (C4H8O2) in a combustion reaction?
A
2.40 g
B
3.20 g
C
4.80 g
D
6.40 g
Verified step by step guidance1
Write the balanced chemical equation for the combustion of butyric acid (C4H8O2). The general form for the combustion of an organic compound is: CxHyOz + O2 -> CO2 + H2O.
Balance the equation by ensuring the number of atoms of each element is the same on both sides. For butyric acid, the balanced equation is: C4H8O2 + 5O2 -> 4CO2 + 4H2O.
Calculate the molar mass of butyric acid (C4H8O2) by adding the atomic masses of all the atoms in the formula: (4 * 12.01 g/mol for C) + (8 * 1.01 g/mol for H) + (2 * 16.00 g/mol for O).
Determine the moles of butyric acid by dividing the given mass (1.33 g) by its molar mass.
Use the stoichiometry from the balanced equation to find the moles of O2 needed. According to the equation, 1 mole of C4H8O2 reacts with 5 moles of O2. Multiply the moles of butyric acid by 5 to find the moles of O2 required, then convert this to grams using the molar mass of O2 (32.00 g/mol).
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