Answer:
The reaction is spontaneous when T> 0.98 Kelvin OR T> -272.17°C
Explanation:
Step 1: Data given
ΔH = 131.3 kJ/mol = 131300 J/mol
ΔS = 133.6 J/K*mol
T = 298K
Step 2: The balanced equation
C (s) + H2O (g) --> CO (g) + H2 (g)
Step 3: ΔG
For a reaction to be spontaneous, ΔG should be <0
When ΔG > 0 the reaction is spontaneous in the reverse direction.
ΔG = ΔH - TΔS
Since ΔG<0
ΔH - TΔS <0
Step 4: Calculate T where the reaction is spontaneous
ΔH - TΔS <0
131300 J/mol - T*133.6 J/K*mol <0
- T*133.6 J/K*mol < -131300 J/mol
-T <-131300 /133.6
-T< -982.8 Kelvin
T> 982.8 Kelvin OR T> 709.6°C
The reaction is spontaneous when T> 982.8 Kelvin OR T> 709.6°C
At 298 K this reaction C (s) + H2O (g) --> CO (g) + H2 (g) is <u>not spontaneous</u>
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Explanation:
To solve this problem, we need to understand the concept of precision and accuracy.
Through this understanding we apply to solve this problem.
- Precision is the ability to reproduce the same set of values in an experiment.
- Accuracy is the nearness or closeness of the measured value to the true value.
For example; if the true value is 28.0mm and the following readings were made:
A = 24.0mm, 24.0mm, 24.3mm, 23.9mm This is a precise measurement but not accurate.
B = 27.9mm, 28.0mm, 28.1mm: This is an accurate measurement because it is close to the true value.
