Be sure to answer all parts. How many liters of the antifreeze ethylene glycol CH,(OH)CH,(OH) | would you add to a car radiator amany containing 6.25 L of water if the coldest winter temperature in your area is -19.0°C? Calculate the boiling point of this water-ethylene glycol mixture. (The density of ethylene glycol is 1.11 g/mL.) What is the volume of antifreeze? What is the boiling point of the solution?

Be sure to answer all parts. How many liters of the antifreeze ethylene glycol CH,(OH)CH,(OH) | would you add to a car radiator amany containing 6.25 L of water if the coldest winter temperature in your area is -19.0°C? Calculate the boiling point of this water-ethylene glycol mixture. (The density of ethylene glycol is 1.11 g/mL.) What is the volume of antifreeze? What is the boiling point of the solution?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The boiling point of chloroform, CHCl3, is 61.700 °C at 1 atmosphere. Kb(chloroform) = 3.67 °C/mIn a laboratory experiment, students synthesized a new compound and found that when 14.17 grams of the compound were dissolved in 258.8 grams of chloroform, the solution began to boil at 62.816 °C. The compound was also found to be nonvolatile and a non-electrolyte.What is the molecular weight they determined for this compound ? _______________g/mol
The freezing point of water H2O is 0.00°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in water is antifreeze (ethylene glycol).How many grams of antifreeze, CH2OHCH2OH (62.10 g/mol), must be dissolved in 267.0 grams of water to reduce the freezing point by 0.400°C ? Refer to the table for the necessary boiling or freezing point constant. _______g antifreeze.
A solution of toluene (C-Hs) in 236 g of cyclohexane (C6H12) has a boiling point of 90.30 °C. What quantity in moles of toluene are in the solution? (For cyclohexane Kb = 2.92 °C/m, normal boiling point, Tb = 80.90 °C)
- 1 A certain liquid X has a normal freezing point of –1.00 °C and a freezing point depression constant K,=2.88 °C·kg•mol *. A solution is prepared by dissolving some zinc chloride (ZnCl,) in 350. g of X. This solution freezes at -2.1 °C. Calculate the mass of ZNC1, that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. alo 18.2 g Ar х10
[References] If we add 178 g of ethylene glycol, C,H,O2, per 1000. g of water to a car radiator, what will be the freezing point of the solution? The Kf for water is 1.86 mol particles °C
The boiling point of water is 100.0°C at 1 atmosphere. How many grams of aluminum chloride (133.3 g/mol), must be dissolved in 253.0 grams of water to raise the boiling point by 0.450 °C? Refer to the table for the necessary boiling or freezing point constant. Solvent Kb (°C/m) Kf(°C/m) Water 0.512 Ethanol 1.22 Chloroform CHCl3 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 g aluminum chloride Mass = Formula H₂O CH3 CH₂OH 1.86 1.99 5.12
A 3.40-g sample of a mixture of naphthalene (C₁₀H₈) and pyrene (C₁₆H₁₀) is dissolved in 35.0 g benzene (C₆H₆). The freezing point of the solution is 2.29°C. What is the mass (in grams) of the naphthalene in the sample mixture? The freezing point of benzene is 5.51°C and Kf is 5.12°C･kg/mol.
Pure water boils at 100 oC. What is the boiling point of a solution (use unit symbol C. Do not include the degree symbol) prepared by dissolving 24.5 g of CaCl2 in 89.6 g of waterat 45.0 ºC, assuming complete dissociation? For water, Kb = 0.51 C.kg/mol. Molar mass calcium chloride = 110.98 g/mol. Give you answer to four sig figs.
A solution of toluene (C,H₂) in 301 g of cyclohexane (CH₁₂) has a boiling point of 90.30 °C. What quantity in moles of toluene are in the solution? (For cyclohexane Kb = 2.92 °C/m, normal boiling point, Tb = 80.90 °C)
The normal boiling point of a certain liquid X is 141.40 °C, but when 20. g of glycine (C,H,NO2) are dissolved in 250. g of X the solution boils at 142.6 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. olo °C·kg K, = ] x10 Ar mol ?
sited [Review Topics] [References] Use the References to access important values if needed for this question. The boiling point of diethyl ether, CH3 CH2 OCH2 CH3, is 34.500 °C at 1 atmosphere. K, (diethyl ether) = 2.02 °C/m In a laboratory experiment, students synthesized a new compound and found that when 10.14 grams of the compound were dissolved in 270.0 grams of diethyl ether, the solution began to boil at 34.714 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol Submit Answer ph_08-30-2....pdf Retry Entire Group a a 9 more group attempts remaining C Previous Next 07 Show all 11:14 PM 9/12/2022