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

conduction is the transfer of thermal energy (heat in transfer) due to collisions between the molecules in the object. collisions between adjacent atoms and molecules transfer kinetic energy from the warmer to the cooler object. the objects must be in physical contact.

a polar bond is formed when electrons are shared unevenly between atoms