if 5.0g zinc reacts with 10.0 g hci to produce h2 gas and znci2 according to the following equation zn=2hci znci2 + h2 what is the limiting reactant and how many grams of h2 will be produced

The mass of produced is 0.153 g

Explanation:

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

......(1)

Given mass of zinc = 5.0 g

Molar mass of zinc = 65.38 g/mol

Putting values in equation 1, we get:

Given mass of HCl = 10.0 g

Molar mass of HCl = 36.46 g/mol

Putting values in equation 1, we get:

The given chemical equation follows:

By stoichiometry of the reaction:

If 1 mole of zinc reacts with 2 moles of HCl

So, 0.0765 moles of zinc will react with = of HCl

As the given amount of HCl is more than the required amount. Thus, it is present in excess and is considered as an excess reagent.

Thus, zinc is considered a limiting reagent because it limits the formation of the product.

By the stoichiometry of the reaction:

If 1 mole of zinc produces 1 mole of

So, 0.0765 moles of zinc will produce = of

We know, molar mass of = 2 g/mol

Putting values in above equation, we get:

Hence, the mass of produced is 0.153 g

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"