Predict the products of the double replacement reaction 2KOH + H2504 --?
1 answer:
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Answer:
A. -166.6 kJ/mol
B. -127.7 kJ/mol
C. -133.9 kJ/mol
Explanation:
Let's consider the oxidation of sulfur dioxide.
2 SO₂(g) + O₂(g) → 2 SO₃(g) ΔG° = -141.8 kJ
The Gibbs free energy (ΔG) can be calculated using the following expression:
ΔG = ΔG° + R.T.lnQ
where,
ΔG° is the standard Gibbs free energy
R is the ideal gas constant
T is the absolute temperature (25 + 273.15 = 298.15 K)
Q is the reaction quotient
The molar concentration of each gas ([]) can be calculated from its pressure (P) using the following expression:
<em>Calculate ΔG at 25°C given the following sets of partial pressures.</em>
<em>Part A 130atm SO₂, 130atm O₂, 2.0atm SO₃. Express your answer using four significant figures.</em>
ΔG = ΔG° + R.T.lnQ = -141.8 kJ/mol + (8.314 × 10⁻³ kJ/mol.K) × 298 K × ln (4.44 × 10⁻⁵) = -166.6 kJ/mol
<em>Part B 5.0atm SO₂, 3.0atm O₂, 30atm SO₃ Express your answer using four significant figures.</em>
<em />
ΔG = ΔG° + R.T.lnQ = -141.8 kJ/mol + (8.314 × 10⁻³ kJ/mol.K) × 298 K × ln 296 = -127.7 kJ/mol
<em>Part C Each reactant and product at a partial pressure of 1.0 atm. Express your answer using four significant figures.</em>
<em />
ΔG = ΔG° + R.T.lnQ = -141.8 kJ/mol + (8.314 × 10⁻³ kJ/mol.K) × 298 K × ln 24.4 = -133.9 kJ/mol
Answer:
The maximum mass of carbon dioxide that could be produced by the chemical reaction is 70.6gCO_{2}
Explanation:
1. Write down the balanced chemical reaction:
2. Find the limiting reagent:
- First calculate the number of moles of hexane and oxygen with the mass given by the problem.
For the hexane:
For the oxygen:
- Then divide the number of moles between the stoichiometric coefficient:
For the hexane:
For the oxygen:
- As the fraction for the oxygen is the smallest, the oxygen is the limiting reagent.
3. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction:
The calculations must be done with the limiting reagent, that is the oxygen.