The reactions involved are synthesis, combustion and single replacement reactions and the masses of products formed are dependent on the mole ratio.
What are limiting reactants?
Limiting reactants are reactants are reactants that are used in a chemical reaction.
The equation for the production of water is given below:
[tex]2H_2 + O_2 \rightarrow 2H_2O[/tex]
The reaction is a synthesis reaction and the mole ratio of hydrogen to oxygen is 2 : 1.
Moles of 250 g of Hydrogen = 250/2 = 125 moles
Moles of water produced = 125 moles
Mass of water = 125 × 18 = 2250 g
Moles of oxygen in 250 g = 250/32 = 7.81 moles
Moles of water produced = 7.81 × 2 = 15.62
Mass of water produced = 15.62 × 18 = 281.16 g
Since moles of oxygen use is less than the mole ratio of reaction, oxygen is the limiting reactant.
2. The reaction of propane and oxygen is a combustion reaction and is given below:
[tex]C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O[/tex]
1 mole of propane produces 4 moles of water
44 g of propane produces 72 g of water
Mass of propane required to produce 1000 g of water = 1000 × 44/ 72 = 611.1 g of propane
3. The reaction of zinc and hydrochloride acid is a single replacement reaction and the equation is given below:
[tex]Zn + 2HCl \rightarrow ZnCl_2 + H_2[/tex]
1 mole of Zn and 2 moles of HCl are required to produce 1 mole of hydrogen gas
Molar mass of Zn = 65 g
Molar mass of HCl = 36.5
Molar mass of hydrogen = 2.0 g
150 g of Hydrogen gas = 150/2 = 75 moles of hydrogen
Mass of 75 moles of Zn = 75 × 65 = 4875 g
mass of 75 × 2 moles if HCl = 150 × 36.5 =5475 g
Therefore, 4875 g of Zn and 5475 g of HCl are required to produce 150 g of Hydrogen gas.
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