A container containing 6.19 L of a gas is collected at 244 K and then allowed...
A container containing 6.19 L of a gas is collected at 244 K and then allowed to expand to 23.4 L. What must the new temperature be in order to maintain the same pressure? Express your answer in units of K. You do not need to enter the unit.
When 16.8-grams of an unknown compound is placed in 0.176-kg of benzene, the freezing point is changed by 1.93oC. The value of Kf= 4.90oC/m for benzene. Determine the molar mass of the unknown compound. Answer to 1 decimal place and include your units.
Determine the molarity of a solution containing 14.2 grams of ethanol, C2H5OH (Molar mass = 46.08 g/mol) dissolved in 1.5 liters of solution. Answer to 2 decimal places.
Determine the osmotic pressure when 94 g of fructose (Molar mass = 180.06 g/mol) is dissolved in enough water to make 725.7 mL of solution at 27.20C. Answer to 2 decimal places and please include your units
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A container containing 6.19 L of a gas is collected at 244 K and
then allowed...
When 12.6-grams of an unknown compound is placed in 0.116-kg of benzene, the freezing point is...
When 12.6-grams of an unknown compound is placed in 0.116-kg of benzene, the freezing point is changed by 2.34°C. The value of Kf= 4.90°C/m for benzene. Determine the molar mass of the unknown compound. Answer to 1 decimal place and include your units. Answer: Determine the molality of a solution when 32.3 grams of ethanol, C2H5OH (Molar mass = 46.08 g/mol) is dissolved in 0.947 kg of water. Answer to 2 decimal places. Answer: Find the freezing point of a...
Determine the molarity of a solution containing 17.2 grams of ethanol, C2H5OH (Molar mass = 46.08...
Determine the molarity of a solution containing 17.2 grams of ethanol, C2H5OH (Molar mass = 46.08 g/mol) dissolved in 3.1 liters of solution. Answer to 2 decimal places.
1.Determine the molarity of a solution that contains 8.4 moles of ethanol dissolved in 4.7 liters...
1.Determine the molarity of a solution that contains 8.4 moles of ethanol dissolved in 4.7 liters of solution. Answer to 2 decimal places. 2.Determine the mole fraction of ethanol, C2H5OH (Molar mass = 46.08 g/mol) when 13.4 grams of ethanol is dissolved in 96.1 grams of water, H2O (Molar mass = 18.02 g/mol).
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is...
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is dissolved in benzene (C6H), an organic solvent. Use the data below to determine the molar mass of the substance. 8.65 g Mass of unknown compound Freezing point of solution Volume of benzene -10.21°C 35.0 mL 5.53°C Freezing point of benzene Density of benzene Kf for benzene 0.8765 g/mL 5.12°C/m Molar mass = g/mol
2. Suppose you just made a compound containing only boron and fluorine. To determine its molar...
2. Suppose you just made a compound containing only boron and fluorine. To determine its molar mass you dissolve 0.176 g in 110.0 g of benzene and find that the freezing point of the solution is 4.77°C. (the freezing point of pure benzene is 5.50°C and K, for benzene is -4.90 °C/molal) If the compound contains 22.1% boron, what are the empirical and molecular formulas of the boron-fluorine compound?
plz answer as soon as possible point depression data allow us to determine how many moles...
plz answer as soon as possible
point depression data allow us to determine how many moles of particles are dissolved in solution. of 0500 grams of unknown and 20.0 grams of benzene freezes at 2.0O Trand K for benzene (see Table in lab procedure) to find the molality (mol/kg) of the solution, moles, and molar mass of the unknown substance? (Tt for Benzene is 5.5°C and Kf - 5.12C m) A 068 m, 36 6 mol, 0.014 g/mol 068 m...
A 5.11 g sample of a compound is dissolved in 154.7 g of benzene. The freezing...
A 5.11 g sample of a compound is dissolved in 154.7 g of benzene. The freezing point of this solution is 1.00°C below that of pure benzene. The compound is a nonelectrolyte. What is the molar mass of this compound? K for benzene = 5.12(°C kg)/mol. (Do not include units in your answer. If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to the nearest whole number.) AT=i Kh Msolute AT...
Remaining Time: 1 hour, 33 minutes, 40 seconds. Question Completion Status: 12 15 13 10 11...
Remaining Time: 1 hour, 33 minutes, 40 seconds. Question Completion Status: 12 15 13 10 11 14 9 8 7 4 5 6 3 2 1 Moving to the next question prevents changes to this answer Question 1 of 15 Question 1 8 points When 60.0 grams of an unknown compound are dissolved in 0.500 kg of benzene, the freezing point of the resulting solution is 126"C. The freezing point of pure benzene is 5.44°C, and the Kffor benzene is...
A solution prepared at 20 degrees celsius by dissolving 7.44g of an unknown hydrocarbon in 75g...
A solution prepared at 20 degrees celsius by dissolving 7.44g of an unknown hydrocarbon in 75g benzene (C6H6, 78.112 g/mol, 0.8765 g/cm^3) is found to have a vapor pressure of 376 mmHg at 60 degrees celsius. The vapor pressure of pure benzene at 60 degrees celsius is 400 mmHg. Determine the molar mass of the unknown compound.
1a: 19.930 g of a non-volatile solute is dissolved in 395.0 g of water. The solute...
1a: 19.930 g of a non-volatile solute is dissolved in 395.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 90°C the vapour pressure of the solution is 521.11 torr. The vapour pressure of pure water at 90°C is 525.80 torr. Calculate the molar mass of the solute (g/mol). 1b: Now suppose, instead, that 19.930 g of a volatile solute is dissolved in 395.0...
When 12.6-grams of an unknown compound is placed in 0.116-kg of benzene, the freezing point is changed by 2.34°C. The value of Kf= 4.90°C/m for benzene. Determine the molar mass of the unknown compound. Answer to 1 decimal place and include your units. Answer: Determine the molality of a solution when 32.3 grams of ethanol, C2H5OH (Molar mass = 46.08 g/mol) is dissolved in 0.947 kg of water. Answer to 2 decimal places. Answer: Find the freezing point of a...
The molar mass of unknown molecular compound is determined using freezing point depression. The substance is dissolved in benzene (C6H), an organic solvent. Use the data below to determine the molar mass of the substance. 8.65 g Mass of unknown compound Freezing point of solution Volume of benzene -10.21°C 35.0 mL 5.53°C Freezing point of benzene Density of benzene Kf for benzene 0.8765 g/mL 5.12°C/m Molar mass = g/mol
2. Suppose you just made a compound containing only boron and fluorine. To determine its molar mass you dissolve 0.176 g in 110.0 g of benzene and find that the freezing point of the solution is 4.77°C. (the freezing point of pure benzene is 5.50°C and K, for benzene is -4.90 °C/molal) If the compound contains 22.1% boron, what are the empirical and molecular formulas of the boron-fluorine compound?
plz answer as soon as possible
point depression data allow us to determine how many moles of particles are dissolved in solution. of 0500 grams of unknown and 20.0 grams of benzene freezes at 2.0O Trand K for benzene (see Table in lab procedure) to find the molality (mol/kg) of the solution, moles, and molar mass of the unknown substance? (Tt for Benzene is 5.5°C and Kf - 5.12C m) A 068 m, 36 6 mol, 0.014 g/mol 068 m...
A 5.11 g sample of a compound is dissolved in 154.7 g of benzene. The freezing point of this solution is 1.00°C below that of pure benzene. The compound is a nonelectrolyte. What is the molar mass of this compound? K for benzene = 5.12(°C kg)/mol. (Do not include units in your answer. If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to the nearest whole number.) AT=i Kh Msolute AT...
Remaining Time: 1 hour, 33 minutes, 40 seconds. Question Completion Status: 12 15 13 10 11 14 9 8 7 4 5 6 3 2 1 Moving to the next question prevents changes to this answer Question 1 of 15 Question 1 8 points When 60.0 grams of an unknown compound are dissolved in 0.500 kg of benzene, the freezing point of the resulting solution is 126"C. The freezing point of pure benzene is 5.44°C, and the Kffor benzene is...
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