Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to the reaction bao 2 ( s ) + h 2 so 4 ( aq ) ⟶ baso 4 ( s ) + h 2 o 2 ( aq ) bao2(s)+h2so4(aq)⟶baso4(s)+h2o2(aq) how many milliliters of 3.00 m h 2 so 4 ( aq ) 3.00 m h2so4(aq) are needed to react completely with 92.5 g bao 2 ( s ) ? 92.5 g bao2(s)?

There is 182 mL of 3.00 M H2SO4 needed

Explanation:

Step 1: Data given

Mass of BaO2 = 92.5 grams

Molarity of 3.00 M H2SO4

Step 2: The balanced equation

BaO2 ( s ) + H2SO4(aq ) ⟶ BaSO4(s) + H2O2(aq )

For 1 mole of BaO2  we need 1 mole of H2SO4 to produce 1 mole of BaSO4 and 1 mole H2SO2

Step 3: Calculate moles of  BaO2

Moles BaO2 = mass BaO2 / Molar mass BaO2

Moles BaO2 = 92.5 / 169.33 g/mol

Moles BaO2 = 0.546 moles

Step 4: Calculate moles of H2SO4

For 1 mole BaO2 we need 1 mole of H2SO4

For 0.546 moles of BaO2 we need 0.546 moles of H2SO4

Step 5: Calculate the volume of H2SO4 needed

Volume = moles / molarity

Volume = 0.546 mol/ 3.00 mol/L

Volume = 0.182 L = 182 mL

There is 182 mL of 3.00 M H2SO4 needed

answer is: c. the experiment shows that the red substance experienced a chemical change.

this is chemical change (chemical reaction), because two new substances are formed (metalig liquid and gas), the atoms are rearranged and the reaction is followed by an energy change.

this is example of chemical decomposition.

chemical decomposition (analysis) is the separation of a single chemical compound into its two or more elemental parts or to simpler compounds.  

chemical decomposition is opposite of chemical synthesis.