Solve During the 9.9 SALE, Otis purchased 1.0 gallon (4.55 L) of antifreeze containing 3.78 L of ethylene glycol for his race car.Assuming that the antifreeze solution only contains ethylene glycol and water, calculate for the following values.Physical PropertiesEthylene Glycol62.068WaterMolar mass, g/molDensity, g/mLFreezing point, °CFreezing point constant (K:), °C/m18.0160.99701.11560.00-12.93.111.861. Calculate the molality of the antifreeze solution.2. Determine the temperature at which the antifreeze solution will start to freeze.3. According to Mang Tani, the temperature for October will drop to -10°C. Will the antifreeze solution protect therace car engine this month?

1. Molality or molal concentration is defined as the number of moles of solute present per kg of…

Answered: During the 9.9 SALE, Otis purchased 1.0…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter7: Equilibria In Multiple-component Systems

Section: Chapter Questions

Problem 7.38E

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ΔHsolution of NaOH(s) Phase Change:Mass of NaOH: 2.330 gΔT for reaction A : 10.0 °C Calculate the total number of calories produced by the solution.help
Use the provided chart for this question. What is the minimum temperature required to dissolve at least 30g of potassium chloride in 100g of water?? 1.10 Celsius 2.20 Celsius 3.30 Celsius 4.40 Celsius 5.50 Celsius??
Ethylene glycol [CH2(OH)CH2(OH)]is a common automobile antifreeze. The freezing point and boiling point of a solution containing 293 g of ethylene glycol and 1085 g of water are ____and _____ respectively. (Kb and Kf for water are 0.52°C/m and 1.86°C/m, respectively) 8.09 to the power of o space end exponent C comma negative 102.3 to the power of o C negative 9.09 to the power of o space end exponent C comma 112.3 to the power of o C negative 6.09 to the power of o space end exponent C comma 108.3 to the power of o C negative 8.09 to the power of o space end exponent C comma 102.3 to the power of o C
A: 4.91 g of LiCl was dissolved in 50.0 mL of water in the same calorimeter as in problem 1. Analysis of the thermogram showed the initial temperature to be 22.9°C, the final temperature to be 49.2°C. Was the dissolution of the ionic solid exothermic or endothermic? B: Using the information above, calculate the mass of the water. C: Calculate ΔHsolution D : Calculate the standard molar enthalpy of solution. Assume that the pressure is 1 bar.
When 2.00 g of sodium hydroxide (NaOH) was dissolved in 150.00 g of water a value of 11.00oC was obtained for ΔT. (molarity is .333) Calculate the value (calories) for the heat of solution of 2.00 g of NaOH.
Most gases become less soluble in water as the temperature increases. What can be concluded about the signs of (Delta H of solution) and (Delta S of solution) in this case?(A) ΔHsoln is negative and ΔSsoln is negative.(B) ΔHsoln is positive and ΔSsoln is negative.(C) ΔHsoln is positive and ΔSsoln is positive.(D) ΔHsoln is negative and ΔSsoln is positive.
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