Jeneen v A certain liquid X has a normal bolling polnt of 120.70 °C and a bolling potnt elevation constant K=2.07 °C-kg-mol. Calculate the bolling point of a solution made of 98.6g of Iron(III) chloride (FeCl) dissolved In 800. g of X. Round you answer to 5 significant digits. O°C

Calculate the vapor pressure of water over a solution made by dissolving 225.0 g of glucose (C6H12O6) in 575 g water at 35°C. (At 35°C 42.2mmHg) P⁰ water ▸ Files ▬ a r D F7 I F8 FQ prt sc F10 home Bun F11 end F12 insert delete

P. The normal boiling point of a certain liquid X is 142.70 °C, but when 0.13 kg of barium hydroxide (Ba(OH),) are dissolved in 750. g of X the solution boils at 144.4°C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. °C-kg OLX = 'x Continue Submit Assignment O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility EPIC MacBook Pro F3 F8 F10 #3 3. $ 8 R. T. A H と alt pubuwo command option

-1 A certain substance X has a normal boiling point of 117.9 °℃ and a molal boiling point elevation constant K₂=2.27 °C.kg-mol O Calculate the boiling point of I a solution made of 49.6 g of urea ((NH₂)₂CO) dissolved in 750. g of X. Round your answer to 4 significant digits. °C x10

When 0.6403 of g calcium bromide is dissolved in 75.00 mL water, the solution temperature increses by 1.07 °C. Calculate the enthalpy of dissolution (ΔHrxn) for calcium bromide, in kj/mol.(Assume constant pressure is, 41.84j/g. °C as the specific heat capacity of the solution, and a density of 1.00 g/ml). Write out the equation.  I am confused on where to start with this problem.

A test tube contains 2.63x10-4 m3 of liquid carbon tetrachloride (β = 1240x10-6 (C°)-1) at a temperature of 80.0°C. The test tube and the carbon tetrachloride are cooled to a temperature of -10.0°C, which is above the freezing point of carbon tetrachloride. Find the volume of carbon tetrachloride in the test tube at -10.0°C.

From your data in Part 1 of the experiment, you calculate the natural log of the partial pressure of water and 1/T value in K for 5 points between 50°C and 80°C. You make a graph of In(P) vs. 1/T and determine that the slope of the linear line is -4800 K. Use this information to calculate AHvap of water. Make sure to use R = 8.314 J mol-1-K-1. Oa. 46.6 kJ/mol Ob. 0.578 kJ/mol Oc. 31.5 kJ/mol O d. 39.9 kJ/mol

Mm.9.

During the cooling of the aqueous KNO3 solution, you will be asked to record the temperature when crystals first appear. What is the condition of the solution when you first noted the crystal formation?

Molar mass of water= 25mL