# G co 6 worksheet #1 writing and balancing formula equations answers

We have more lessons on the rules for balancing chemical equations. Common abbreviations include s for solids, l for liquids, g for gases, and aq for substances dissolved in water aqueous solutions, as introduced in the preceding chapter.

When calcium comes in contact with water, calcium hydroxide and hydrogen gas is produced. Dividing each coefficient by the greatest common factor, 3, gives the preferred equation: Use this interactive tutorial for additional practice balancing equations.

Zinc hydroxide reacts with phosphoric acid H3PO4 to produce zinc phosphate and water. The following table gives the physical states and the state symbols used in chemical equations: solid, liquid, gas, aqueous. Other examples of these special conditions will be encountered in more depth in later chapters. Sometimes, state symbols are required to indicate the physical states of the substances in a chemical reaction.

## Writing and balancing chemical equations worksheet answers pdf

Sodium Chloride solution and insoluble iron II hydroxide are produced. Additional Information in Chemical Equations The physical states of reactants and products in chemical equations very often are indicated with a parenthetical abbreviation following the formulas. Write balanced molecular, complete ionic, and net ionic equations for this process. Step 2: Balance the chemical equation. Every chemical change can be communicated symbolically using a chemical equation. Explicitly representing all dissolved ions results in a complete ionic equation. Place them based on the chemical equation and write the state symbols. Chemical Equation A chemical equation shows the overall change of reactants to products in a chemical reaction. For example, consider the reaction of ethane C2H6 with oxygen to yield H2O and CO2, represented by the unbalanced equation: Following the usual inspection approach, one might first balance C and H atoms by changing the coefficients for the two product species, as shown: This results in seven O atoms on the product side of the equation, an odd number—no integer coefficient can be used with the O2 reactant to yield an odd number, so a fractional coefficient, , is used instead to yield a provisional balanced equation: A conventional balanced equation with integer-only coefficients is derived by multiplying each coefficient by 2: Finally with regard to balanced equations, recall that convention dictates use of the smallest whole-number coefficients. When compounds react, they are chemically changed into new compounds. Although the equation for the reaction between molecular nitrogen and molecular hydrogen to produce ammonia is, indeed, balanced, the coefficients are not the smallest possible integers representing the relative numbers of reactant and product molecules. When ionic compounds dissolve in water, they may dissociate into their constituent ions, which are subsequently dispersed homogenously throughout the resulting solution a thorough discussion of this important process is provided in the chapter on solutions. Phosphorous reacts with oxygen gas to produce diphosphorous pentoxide. Example 2 Molecular and Ionic Equations When carbon dioxide is dissolved in an aqueous solution of sodium hydroxide, the mixture reacts to yield aqueous sodium carbonate and liquid water.

Sodium hydroxide reacts with iron III nitrate to create a precipitate of iron III hydroxide in a solution of sodium nitrate.

To illustrate this, consider a reaction between ionic compounds taking place in an aqueous solution. When hexane C6H24 reacts with oxygen a combustion reaction occurs.

Step 3: Balance the chemical equation. When ionic compounds dissolve in water, they may dissociate into their constituent ions, which are subsequently dispersed homogenously throughout the resulting solution a thorough discussion of this important process is provided in the chapter on solutions.

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