what is the molarity of 8.63 g benzene (C6H6) dissolved in 23.8 g carbon tetrachloride (CCl4)

Expert Solution

queen_honey_blossom answered 2 years ago

A solution has a 0.102 mole fraction of benzene (C6H6) in carbon tetrachloride (CCl4). The density...

A solution has a 0.102 mole fraction of benzene (C6H6) in carbon tetrachloride (CCl4). The density of the solution is 1.55 g/mL. The molar masses of benzene and carbon tetrachloride are 78.1 g/mol and 154 g/mol respectively. What is the mass percent, molarity and molality of the benzene?

how many molecules of carbon tetrachloride are there in 80g of ccl4 sample

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The vapor pressure of pure carbon tetrachloride, CCl4, (molar mass 153.82 g/mol) is 0.354 atm, and the vapor pressure of pure chloroform, CHCl3 (molar mass 119.38 g/mol), is 0.526 atm at 316 K. A solution is prepared from equal masses of the two compounds at this temperature. If the vapor over the original solution is condensed and isolated into a separate flask, what with the vapor pressure of the chloroform be above this new solution?

Carbon tetrachloride, CCl4, was once used as a dry cleaning solvent, but is no longer used...

Carbon tetrachloride, CCl4, was once used as a dry cleaning solvent, but is no longer used because it is carcinogenic. At 57.8 °C, the vapor pressure of CCl4 is 0.530 atm, and its enthalpy of vaporization is 33.05 kJ/mol. Use this information to estimate the normal boiling point for CCl4. please show work

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A gaseous mixture containing 0.170 mol fraction of carbon tetrachloride (CCl4) and 0.830 mol fraction of...

A gaseous mixture containing 0.170 mol fraction of carbon tetrachloride (CCl4) and 0.830 mol fraction of dry air is initially at 61.0°C and 1037 mmHg. If this mixture is cooled at a constant pressure, at what temperature does the CCl4 first start to condense? At what temperature would 44.0% of the CCl4 condense?

If 0.10 g of benzene (C6H6) is ignited in a 0.3 L vessel at 298K and...

If 0.10 g of benzene (C6H6) is ignited in a 0.3 L vessel at 298K and surrounded by 25 atm of oxygen: a) Write the net reaction; b) How many moles of O2 were consumed?; c) How many moles of product were produced?; d) What is the change in moles in the reaction vessel?; e) Assuming all of the products were ideal gas what is the new pressure in the container?; f) What is the work done by this reaction?;...

A solution consists of 3.88 g benzene,C6H6 , and 2.45 g toluene ,C6H5CH3. The vapor pressure...

A solution consists of 3.88 g benzene,C6H6 , and 2.45 g toluene ,C6H5CH3. The vapor pressure of pure benzene at 20. °C is 75 mm Hg and that of toluene at 20.0 °C is 22 mm Hg. Assume that Raoult’s lawholds for each component of the solution, calculate the mole fraction of benzene in the vapor. ( molar mass of benzene= 78.0 g/mole and toluene = 92.0 g/mole.) Answer= 0.87

50 grams of benzene (C6H6) is placed in a containr with 160 g of oxygen gas....

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Within 100 g of pure benzene (C6H6) with freezing and boiling temperatures of 5.5 oC and 80.1 oC respectively 24.4 g of biphenyl (C12H10) dissolves. Benzene freezing point lowering and boiling point rise constants 5.12 K kg mol-1 and 2.63 K kg mol-1 According to the solution at 80.1 oC Find the freezing and boiling temperatures of the solution as well as the vapor pressure. (Your normal gasoline steam pressure at boiling temperature of 80.1 oC p1 o = 760...

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