You cannot change the subscripts in the molecular identities.
For example, H2SO4 must remain H2SO4 and not changed to something like H3SO7.
Furthermore, the total mass of the reactants must equal the total mass of the products.
The number and type of atoms must always remain the same on both sides of the equation when balancing a chemical equation. This requirement is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.
false
The chemical formulas of the reactants and products cannot be changed when balancing a chemical equation. The Law of Conservation of Mass states that matter cannot be created or destroyed in a chemical reaction, so the number of atoms of each element on both sides of the equation must be equal.
True. Subscripts represent the number of atoms of each element in a compound and changing them would change the chemical formula, possibly making it unbalanced in the equation. By adjusting the coefficients of the compounds involved in the reaction, the equation can be balanced without modifying the subscripts.
Coefficients can be adjusted to balance a chemical equation. Coefficients are placed in front of chemical formulas to ensure that there is the same number of each type of atom on both sides of the equation. The goal is to have an equal number of atoms of each element on the reactant and product sides.
A constant
No, subscripts cannot be changed in a chemical formula to balance a chemical equation. Balancing a chemical equation involves adjusting the coefficients in front of the chemical formulas to ensure that the number of each type of atom is the same on both sides of the equation. Changing subscripts would alter the chemical identities of the substances involved.
The number and type of atoms must always remain the same on both sides of the equation when balancing a chemical equation. This requirement is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.
false
The chemical formulas of the reactants and products cannot be changed when balancing a chemical equation. The Law of Conservation of Mass states that matter cannot be created or destroyed in a chemical reaction, so the number of atoms of each element on both sides of the equation must be equal.
True. Subscripts represent the number of atoms of each element in a compound and changing them would change the chemical formula, possibly making it unbalanced in the equation. By adjusting the coefficients of the compounds involved in the reaction, the equation can be balanced without modifying the subscripts.
Coefficients can be adjusted to balance a chemical equation. Coefficients are placed in front of chemical formulas to ensure that there is the same number of each type of atom on both sides of the equation. The goal is to have an equal number of atoms of each element on the reactant and product sides.
A coefficient is the number that goes before an element when your balancing the equation. And a subscript is the number after the element. Subscripts are not changed when you balance the equation.
The law that states that the number of atoms on the right side of a chemical equation must be equal to the number of atoms on the left side is the Law of Conservation of Mass. This fundamental principle in chemistry indicates that matter cannot be created or destroyed in a chemical reaction, only rearranged.
The coefficient times the subscripts in a chemical formula show you the number of atoms of each element for each substance in the equation.
The law of conservation of mass is shown by a balanced chemical equation, which states that matter cannot be created or destroyed in a chemical reaction. This means that the number of atoms of each element must be the same on both sides of the equation.
Equations for chemical reactions may require one or more whole-number coefficients in order for the equation to balance. Balancing a chemical equation upholds the law of conservation of mass, which states that matter cannot be created or destroyed. The coefficients represent molar ratios of reactants and products. Performing stoichiometric calculations is largely dependent upon these correct molar proportions.