64.61 kJ of energy is released by the combustion of 16.0 oz of hydrogen
<h3>Further explanation</h3>Delta H reaction (ΔH) is the amount of heat/heat change between the system and its environment
(ΔH) can be positive (endothermic = requires heat) or negative (exothermic = releasing heat)
The reaction of a substance with oxygen is called a combustion reaction
the combustion of hydrogen is
<h3>2H₂ + O₂ → 2H₂O.</h3>This equation shows that 2 Hydrogen molecules react with 1 molecule of oxygen to produce 2 molecules of water
In this combustion reaction will produce large thermal energy because it involves breaking the hydrogen gas bond, so the reaction is exothermic
The combustion of hydrogen releases 142 j / g of hydrogen reacted.
Combustion of 16.0 oz of hydrogen will release heat of:
16 oz = 1 lb = 0.455 kg = 455 g
For each gram Hydrogen releases 142 J, then for 455 g releases:
142 x 455 J = 64610 J = 64.61 kJ
<h3>Learn more</h3>the complete combustion of methane
grams of o2 are required to burn 17.0 gal of c8h18
moles of oxygen are required to produce 2.33 moles of water
Keywords: Combustion of hydrogen, ΔH reaction, water, oxygen, exothermic
Answer: 31.8 g
Explanation:
To calculate the moles :
According to stoichiometry :
1 mole of require 3 moles of
Thus 0.59 moles of will require=
of
Thus is the limiting reagent as it limits the formation of product and
is the excess reagent as it is present in more amount than required.
As 1 mole of give = 2 moles of
Thus 0.59 moles of give =
of
Mass of
Thus 31.8 g of will be produced from the given masses of both reactants.