In aqueous reactions, if the amounts of reactants (and products) that are used are not given in moles, they are usually given in?
volumes
or grams?
In aqueous reactions, if the amounts of reactants (and products) are not given in moles, they are usually given in units of mass, such as grams or kilograms.
To determine the amounts of reactants or products in a given aqueous reaction, you usually need to know the molar mass of the substances involved. The molar mass is the mass of one mole of a substance and is usually expressed in grams per mole (g/mol).
To find the molar mass of a substance, you can look up its atomic masses on the periodic table and sum them up according to the chemical formula. For example, to find the molar mass of water (H2O), you would sum the atomic masses of two hydrogen atoms (1.0079 g/mol each) and one oxygen atom (16.00 g/mol), resulting in a molar mass of 18.015 g/mol.
Once you know the molar mass of a substance, you can convert the given mass into moles using the equation:
moles = mass (in grams) / molar mass (in g/mol)
For example, if you are given 10 grams of water, you can convert it into moles using the molar mass of water (18.015 g/mol):
moles = 10 g / 18.015 g/mol = 0.554 mol
By converting the given mass into moles, you can then use the balanced chemical equation of the reaction to determine the stoichiometric ratios between the reactants and products and calculate the amounts of other substances involved.