Based on the figure above, what is the boiling point (°C) of water under an external pressure of 0.724 atm?

What is the molal concentration of potassium bromide in a solution prepared by dissolving 2.27 g of potassium bromide in 897 g of water?

The enthalpy change for converting 1.00 mol of ice at -25.0 °C to water at 50.0 °C is  The specific heats of ice, water, and steam are   and  respectively. For H2O, ΔHfus = 6.01 kJ/mol, and .

The solubility of oxygen gas in water at 25 °C and 1.0 atm pressure of oxygen is 0.041 g/L.  The solubility of oxygen in water at 4.0 atm and 25 °C is ________ g/L.

A ice sample starts at -30

For the following question, you can receive a majority of points by drawing an appropriate sketch with important information on it.  To receive full credit, you need to answer the quantitative questions.

Answer the following questions about a solution made by dissolving 11.0 g of an unknown non-electrolyte substance in 119 g water at 20°C. Write all answers in decimal format and pay attention to significant figures (don’t include units)!   If the osmotic pressure of this solution was found to be 6.19 atm, what is the concentration of this solution (in M)?   If the density of the solution is 1.04 g/mL, what is the volume of solution (in mL)?   How many moles of solute are present in the solution?   What is the molar mass of the solute (in g/mol)?

Calculate the freezing point of a 0.09500 m aqueous solution of glucose. The molal freezing-point-depression constant of water is 

What must happen before the blood level of a nutrient decrease?

You live in the newest dorm Dejope Hall that houses 500 students. The daily calcium intakes of Dejope residents are listed below: 50 students: 1000 mg; For this population, EAR=800 mg, RDA=1000 mg. The prevalence of inadequate calcium intake in the Dejope Hall is