given the mass lost during the reaction when the alka seltzer is the limiting reagent and that the molar mass of carbon dioxide
1 answer:
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Answer:
Take a look at the attachment below
Explanation:
Take a look at the periodic table. As you can see, Rubidium is the closest element to Cesium, and happens to have the closest boiling point to Cesium, with only a difference of about 30 degrees.
Respectively, you would think that fluorine should have the least similarity to Cesium with respect to it's boiling point, considering it is the farthest away from the element out of the 4 given. This is not an actual rule, there are no fixed trends of boiling points in the periodic table, there are some but overall the trends vary. However in this case fluorine does have the least similarity to Cesium with respect to it's boiling point, a difference of about 1,546.6 degrees.
<em>Hope that helps!</em>
<u>Answer:</u> The freezing point of solution is -117.54°C and the boiling point of solution is 80.48°C
<u>Explanation:</u>
To calculate the mass of ethanol, we use the equation:
Density of ethanol = 0.789 g/mL
Volume of ethanol = 96.3 mL
Putting values in above equation, we get:
- <u>Calculating the freezing point:</u>
Depression in freezing point is defined as the difference in the freezing point of pure solution and freezing point of solution.
The equation used to calculate depression in freezing point follows:
To calculate the depression in freezing point, we use the equation:
Or,
where,
Freezing point of pure solution = -114.1 °C
i = Vant hoff factor = 1 (For non-electrolytes)
= molal freezing point elevation constant = 1.99°C/m
= Given mass of solute (ethylene glycol) = 8.15 g
= Molar mass of solute (ethylene glycol) = 62 g/mol
= Mass of solvent (ethanol) = 75.98 g
Putting values in above equation, we get:
Hence, the freezing point of solution is -117.54°C
- <u>Calculating the boiling point:</u>
Elevation in boiling point is defined as the difference in the boiling point of solution and freezing point of pure solution.
The equation used to calculate elevation in boiling point follows:
To calculate the elevation in boiling point, we use the equation:
Or,
where,
Boiling point of pure solution = 78.4°C
i = Vant hoff factor = 1 (For non-electrolytes)
= molal boiling point elevation constant = 1.20°C/m.g
= Given mass of solute (ethylene glycol) = 8.15 g
= Molar mass of solute (ethylene glycol) = 62 g/mol
= Mass of solvent (ethanol) = 75.98 g
Putting values in above equation, we get:
Hence, the boiling point of solution is 80.48°C