If 34.3 grams of pb02 react how many grams of water will be formed

5.15 g of water

Assuming the reaction in question is the one that occurs in lead storage batteries;

Pb + PbO₂ + 2H⁺ + 2HSO₄⁻ → 2PSO₄ + 2H₂O

The reaction is balanced.

We are given 34.3 grams of PbO₂

Required to determine the mass of water that will be formed,

We can use the following steps;

To get the number of moles we divide mass by the molar mass

Molar mass of PbO₂ = 239.2 g/mol

Therefore;

Moles = 34.3 g ÷ 239.2 g/mol

         = 0.143 moles

From the equation, 1 mole of PbO₂ reacts to produce 2 moles of water.

Therefore, 0.143 moles of PbO₂ would produce,

= 0.143 moles × 2

= 0.286 moles

To get mass we multiply number of moles by the molar mass

Molar mass of water = 18.02 g/mol

Therefore,

Mass = 0.286 moles × 18.02 g/mol

        = 5.154 g

       = 5.15 g

Therefore, 5.15 g of water will be formed

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.

2b2t

explanation:

2b2t