$$ (1\, CO_2\, molecule\, \times \fracO_2\,⟶\,3H_2O\,+\,2CO_2$$Ī conventional balanced equation with integer-only coefficients is derived by multiplying each coefficient by 2:įinally with regard to balanced equations, recall that convention dictates the use of the smallest whole-number coefficients. For example, both product species in the example reaction, CO 2 and H 2O, contain the element oxygen, and so the number of oxygen atoms on the product side of the equation is If an element appears in more than one formula on a given side of the equation, the number of atoms represented in each must be computed and then added together. Note that the number of atoms for a given element is calculated by multiplying the coefficient of any formula containing that element by the element’s subscript in the formula. It may be confirmed by simply summing the numbers of atoms on either side of the arrow and comparing these sums to ensure they are equal. This is a requirement the equation must satisfy to be consistent with the law of conservation of matter. The chemical equation described above is balanced, meaning that equal numbers of atoms for each element involved in the reaction are represented on the reactant and product sides.
