Question

Consider the equation for the formation of water. 2h2 o2 2h2o what is the theoretical yield of h2o if 130 g of h2o is produced from 18 g of h2 and an excess of o2? 18 g 81 g 130 g 160 g

Answer 1

The theoretical yield of 18 gram of  $H_{2}$  is 162 gram of  $H_{2} O$  .

The amount of a product produced by a reaction is generally expressed as a percentage of the reaction's yield. The amount of product that stoichiometry predicts is known as the theoretical yield, but the amount that would be actually achieved is known as the actual yield.

The balanced chemical equation is :

$2H_{2} +O_{2}$  → $2H_{2} O$

It is known that the molar mass of water is 18 gram /mol and 2 gram per mole of $H_{2}$.

18g $H_{2}$ (1 mol  $H_{2}$ (/2 g  $H_{2}$ ()(2 mol  $H_{2} O$  / 2 mol  $H_{2}$ ()(18 g  $H_{2} O$  /1 mol  $H_{2} O$  ) = 162 g $H_{2} O$  .

Theoretical yield will be 162 gram.

So, the theoretical yield of 18 gram of  $H_{2}$  is 162 gram of  $H_{2} O$  .

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