Table of enthalpy of solution for selected cesium salts
Compound and ΔsolH kJ mol-1:
- Cesium bromide: 25.98
- Cesium iodide: 33.35
- Cesium chloride: 17.78
- Cesium fluoride monohydrate: -10.46
- Cesium fluoride sesquihydrate (·1.5H2O): -5.44
Data taken from CRC Handbook of Chemistry and Physics.
Using the information in the above table and the qualitative trends you observed for Part A and the data that you measured in Part B, make a prediction about the rough value of ΔsolH for cesium fluoride (anhydrous). Explain your reasoning process and what evidence you have relied upon in coming to your conclusion.
qerqe
I just used deductive reasoning, that the difference between CsF. 1.5 H2O and CsF 1H2O ... and good luck with Preparation Quiz Experiment 4: So You Want to Conduct?
Yeah have fun, I am struggling with this too.
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To make a prediction about the approximate value of ΔsolH for cesium fluoride (anhydrous), we can analyze the qualitative trends observed for the other cesium salts and consider the evidence from the data provided.
Based on the table, we can observe the following qualitative trends for the ΔsolH of cesium salts:
1. Cesium bromide has the highest ΔsolH value (25.98 kJ mol-1).
2. Cesium iodide has a higher ΔsolH value (33.35 kJ mol-1) than cesium bromide.
3. Cesium chloride has a lower ΔsolH value (17.78 kJ mol-1) than cesium bromide.
4. Cesium fluoride monohydrate has a negative ΔsolH value (-10.46 kJ mol-1), indicating an exothermic dissolution process.
5. Cesium fluoride sesquihydrate (·1.5H2O) also has a negative ΔsolH value (-5.44 kJ mol-1), suggesting an exothermic dissolution process.
Considering these trends, we can make an inference about the rough value of ΔsolH for cesium fluoride (anhydrous). Since cesium fluoride monohydrate and cesium fluoride sesquihydrate both have negative ΔsolH values, it suggests that cesium fluoride's anhydrous form is also likely to have a negative ΔsolH value.
However, due to the lack of specific data for cesium fluoride (anhydrous) in the provided table, we cannot determine the exact value of ΔsolH. To obtain a more accurate prediction, we would need specific experimental data or consult additional references beyond the provided CRC Handbook of Chemistry and Physics.
In summary, based on the observations of the qualitative trends and the evidence from the data provided, we can predict that cesium fluoride (anhydrous) is likely to have a negative ΔsolH value, indicating an exothermic dissolution process.