In the second and third parts of the freezing point depression lab, a solute is added to the test tube containing the solvent by pouring it in from a folded piece of weighing paper. If some of the solute is lost between the weighing and the transfer into the solvent, what effect would this have on your experimental molar mass? Explain your answer.

7. Carbon monoxide gas is found to be more soluble in water than hydrogen gas, even though carbon monoxide and hydrogen gas have very similar Lewis structures. Why? What does have similar Lewis structures have to do with the solubility if any between carbon monoxide and nitrogen? 8. What accounts for a meniscus when measuring liquids in the lab? Explain. Chemical Phases and Vapor Pressure: 9. If the temperature of a liquid is increased, what is the effect on the vapor pressure? 10. The vapor pressure of molecule X at 21.7 °C is 35 mmHg. Find the vapor pressure of this molecule at 68°C. AHvap= 26 kJ/mol, R = 8.314 J/mol*K. Chemical Phases and Heat: 11. How does the heat of fusion of chloroform and the heat of fusion of ethane compare? Why? 130

3. Why is molality and not molarity used to express concentration in the equations for freezing point depression and boiling point elevation?

Predict what will be observed in each experiment below. experiment Two 250 mL samples of water are drawn from a deep well bored into a large underground salt (NaCl) deposit. Sample #1 is from the top of the well, and is initially at 42 °C. Sample #2 is from a depth of 150 m, and is initially at 8 °C. Both samples are allowed to come to room temperature (20 °C) and 1 atm pressure. An NaCl precipitate is seen to form in Sample #1. predicted observation (choose one) A bigger mass of NaCl precipitate will form in Sample #2. A smaller mass of NaCl precipitate will form in Sample #2. The same mass of NaCl precipitate will form in Sample #2. No precipitate will form in Sample #2. O I need more information to predict whether and how much precipitate will form in Sample #2. A student has two unopened 33 cL cans containing carbonated water. Can A has been stored in the garage (32 °C) and can B has been stored in the fridge (8 °C). The student opens one can at the time, both cans make a fizz. O…

In which solvent would the following solute be most likely to dissolve? H. O H-ö-H .. H O H H-C-C-Ç-H H H H HH H H H-C-C-Ç-C-C-Ç-H H H H H H H H. H-C-OH I-O-I I-O-I I I-Ú- I I-Ú -I

help  please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working

please do 9 and 10

I add a non-volatile solute to a pure solvent to form a solution. Will the vapor pressure of this newly formed solution be lower than that of the pure solvent at the PURE SOLVENT's normal boiling point?

In 200 words or less, give a real-world example of a colligative property of a solvent.  How does mixing a solution with a solvent change the physical properties of that solvent. For example, salt is placed on ice on a snowy day to decrease the freezing point of the ice, preventing it from melting and becoming slick and causing accidents.  The colligative property here is freezing point depression.

For results/conclusions Using the images attached Write 2 paragraphs 1st paragraph: Starts with Objective. Results of DeltaT and i stated 2nd paragraph: sources of errors discussed The objective is The colligative properties are the properties that undergo a change when a solute is introduced to a solvent. Freezing point depression is also a colligative property. The addition of a solute to a solvent reduces the freezing point of the resulting solution. The freezing point of the solution is always lower than the freezing point of the solvent. This difference in the freezing point between solvent and solution is called freezing point depression. The freezing point depression is directly proportional to the molality of the solution or the number of moles of solute present in the solution.