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DeltaH=30kJmol^(-1), DeltaS=75J//K//mol....

`DeltaH=30kJmol^(-1), DeltaS=75J//K//mol.
"find boiling temperature at" 1atm: `

A

400K

B

300K

C

150 K

D

425 K

Text Solution

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The correct Answer is:
To find the boiling temperature at 1 atm given the values of ΔH and ΔS, we can follow these steps: ### Step-by-Step Solution: 1. **Understand the Conditions**: At the boiling point, the system is in equilibrium, which means that the Gibbs free energy change (ΔG) is equal to zero. 2. **Use the Gibbs Free Energy Equation**: The relationship between ΔG, ΔH, and ΔS is given by the equation: \[ \Delta G = \Delta H - T \Delta S \] At the boiling point, we set ΔG to zero: \[ 0 = \Delta H - T \Delta S \] 3. **Rearrange the Equation**: Rearranging the equation gives us: \[ T \Delta S = \Delta H \] Therefore, we can solve for T: \[ T = \frac{\Delta H}{\Delta S} \] 4. **Substitute the Values**: We have the following values: - ΔH = 30 kJ/mol = 30,000 J/mol (since 1 kJ = 1000 J) - ΔS = 75 J/K·mol Now substituting these values into the equation: \[ T = \frac{30,000 \, \text{J/mol}}{75 \, \text{J/K·mol}} \] 5. **Calculate the Temperature**: Perform the division: \[ T = 400 \, \text{K} \] 6. **Conclusion**: The boiling temperature at 1 atm is 400 K. ### Final Answer: The boiling temperature at 1 atm is **400 K**.

To find the boiling temperature at 1 atm given the values of ΔH and ΔS, we can follow these steps: ### Step-by-Step Solution: 1. **Understand the Conditions**: At the boiling point, the system is in equilibrium, which means that the Gibbs free energy change (ΔG) is equal to zero. 2. **Use the Gibbs Free Energy Equation**: The relationship between ΔG, ΔH, and ΔS is given by the equation: \[ ...
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Knowledge Check

  • For a given reaction, DeltaH = 35.5 kJ mol^(-1) and Delta S = 83.6 JK^(-1) mol^(-1) . The reaction is spontaneous at (Assume that DeltaH and DeltaS do not vary with temperature)

    A
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    B
    Tgt 425 K
    C
    All temperatures
    D
    Tgt 298 K
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