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One can find the percentage of the mass of a compound that comes from each of the elements in the compound by using this equation: % element =. (number of atoms)(atomic weight) (FW of the compound) x 100.
It takes practice to be able to write balanced equations. There are essentially three steps to the process: 1. Write the unbalanced equation. Chemical formulas of reactants are listed on the left side of the equation. Products are listed on the right side of the equation.
Anatomy of a Chemical Equation. CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g) Coefficients are inserted to balance the equation. Subscripts and Coefficients Give Different Information.
This chapter will describe how to symbolize chemical reactions using chemical equations, how to classify some common chemical reactions by identifying patterns of reactivity, and how to determine the quantitative relations between the amounts of substances involved in chemical reactions—that is, the reaction stoichiometry.
EXAMPLE: Balance on a mixing unit. An aqueous solution of sodium hydroxide contains 20% NaOH by mass. It is desired to produce an 8% NaOH solution by diluting a stream of the 20% solution with a stream of pure water. Calculate the ratios (g H2O/g feed solution) and (g product solution/g feed solution).
Equation (3.2) written for any component component balance. When total mass/material balance is referred, Equation (3.2) is valid for systems involving no chemica reactions as well as those involving chemical reactions.
When multiple reactions occur in a system, an overall stoichiometric equation can be written as a linear combination of the stoichiometric equations. This is possible if, and only if, the ratios between the rates of all reactions remain at constant values whatever the external conditions.
