<h3>
Answer:</h3>
2Fe(s) + 3H₂SO₄ → Fe₂(SO₄)₃ + 3H₂(g)
<h3>
Explanation:</h3>
The equation for the reaction between iron metal and sulfuric acid is given by;
Fe(s) + H₂SO₄ → Fe₂(SO₄)₃ + H₂(g)
We are supposed to balance the equation:
What do we mean by balancing a chemical equation?
- Balancing a chemical equations means that we want to make sure the number of atoms of each element is the same on both sides of the equation.
How is balancing done?
- Balancing of chemical equations is try and error process that is done by putting appropriate coefficients on the reactants and products to equate the number of atoms of each element.
Why are subscripts on the compounds not changed?
- Subscripts in a compound show the actual number of atoms of each element in the compound and therefore can never be altered with because it will distort the chemical compound.
Why is it necessary to balance chemical equations?
- Chemical equations are balanced for them to obey the law of conservation of mass.
- According to this law, the mass of the reactants should be equal to the mass of products, which is achieved through balancing an equation.
What is the required balanced equation?
- The equation given can be balanced by putting the coefficients 2, 3, 1, 3 in that order on the reactants and products.
- Therefore, the balanced chemical equation is;
2Fe(s) + 3H₂SO₄ → Fe₂(SO₄)₃ + 3H₂(g)
Answer:2 AL + FEN2 = 2 ALN + FE
Explanation: AL might be an improperly capitalized: Al. One of your compounds is AL (A and L). Did you mean Al (aluminum)?
FEN2 might be an improperly capitalized: FeN2. ALN might be an improperly capitalized: AlN
FE might be an improperly capitalized: Fe
Answer:
The energies of combustion (per gram) for hydrogen and methane are as follows: Methane = 82.5 kJ/g; Hydrogen = 162 kJ/g
<em>Note: The question is incomplete. The complete question is given below:</em>
To compare the energies of combustion of these fuels, the following experiment was carried out using a bomb calorimeter with a heat capacity of 11.3 kJ/℃. When a 1.00-g sample of methane gas burned with
<em>excess oxygen in the calorimeter, the temperature increased by 7.3℃. When a 1.00 g sample of hydrogen gas was burned with excess oxygen, the temperature increase was 14.3°C. Compare the energies of combustion (per gram) for hydrogen and methane.</em>
Explanation:
From the equation of the first law of thermodynamics, ΔU = Q + W
Since there is no expansion work in the bomb calorimeter, ΔU = Q
But Q = CΔT
where C is heat capacity of the bomb calorimeter = 11.3
kJ/ºC; ΔT = temperature change
For combustion of methane gas:
Q per gram = (
11.3
kJ/ºC * 7.3°C)/1.0g
Q = 83 kJ/g
For combustion of hydrogen gas:
Q per gram = (
11.3
kJ/ºC * 14.3°C)/1.0g
Q = 162 kJ/g
