what would be the total mass of the products of a reaction in which 10 grams of water decomposes into hydrogen and oxygen (and n
2 answers:
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Answer:
ΔS = +541.3Jmol⁻¹K⁻¹
Explanation:
Given parameters:
Standard Entropy of Fe₂O₃ = 90Jmol⁻¹K⁻¹
Standard Entropy of C = 5.7Jmol⁻¹K⁻¹
Standard Entropy of Fe = 27.2Jmol⁻¹K⁻¹
Standard Entropy of CO = 198Jmol⁻¹K⁻¹
To find the entropy change of the reaction, we first write a balanced reaction equation:
Fe₂O₃ + 3C → 2Fe + 3CO
To calculate the entropy change of the reaction we simply use the equation below:
ΔS = ∑S - ∑S
Therefore:
ΔS = [(2x27.2) + (3x198)] - [(90) + (3x5.7)] = 648.4 - 107.1
ΔS = +541.3Jmol⁻¹K⁻¹
<u>Answer:</u> The final temperature of the mixture is 49°C
<u>Explanation:</u>
To calculate the mass of water, we use the equation:
- <u>For cold water:</u>
Density of cold water = 1 g/mL
Volume of cold water = 230.0 mL
Putting values in above equation, we get:
- <u>For hot water:</u>
Density of hot water = 1 g/mL
Volume of hot water = 120.0 mL
Putting values in above equation, we get:
When hot water is mixed with cold water, the amount of heat released by hot water will be equal to the amount of heat absorbed by cold water.
The equation used to calculate heat released or absorbed follows:
......(1)
where,
q = heat absorbed or released
= mass of hot water = 120 g
= mass of cold water = 230 g
= final temperature = ?°C
= initial temperature of hot water = 95°C
= initial temperature of cold water = 25°C
c = specific heat of water = 4.186 J/g°C
Putting values in equation 1, we get:
Hence, the final temperature of the mixture is 49°C