A beaker whose mass was #345.8*g# was filled with a #225*mL# volume of carbon tetrachloride, to give a combined mass of #703.55*g#. Given these data, what is #rho_"carbon tetrachloride"#?

Question

A beaker whose mass was #345.8*g# was filled with a #225*mL# volume of carbon tetrachloride, to give a combined mass of  #703.55*g#.  Given these data, what is #rho_"carbon tetrachloride"#?

Natalie Anton · Accepted Answer

#rho_"carbon tetrachloride"="Mass of carbon tetrachloride"/"Volume of carbon tetrachloride"#

Thus, we entered the following numbers:

#rho_"carbon tetrachloride"=(703.55*g-345.8*g)/(225*mL)=??g*mL^-1#

Because #1*g*mL^-1=1xx10^-3kg*(10^-3L)^-1=1xx10^-3kgxx10^3*L^-1=kg*L^-1#, the #"density"# has the same figures in #kg*L^-1#.

#"Carbon tetrachloride"# will form an immiscible layer with water. Will it float? How can you tell from these figures?

Avery Adams · Answer

undefined The formula to find the density (rho) of carbon tetrachloride is: Density = Mass / Volume. First, calculate the mass of the carbon tetrachloride alone: Mass of carbon tetrachloride = Combined mass - Mass of empty beaker Mass of carbon tetrachloride = 703.55 g - 345.8 g = 357.75 g. Next, use the given volume: Volume of carbon tetrachloride = 225 mL = 225 cm^3. Finally, use the density formula to find the density: Density of carbon tetrachloride = Mass of carbon tetrachloride / Volume of carbon tetrachloride Density of carbon tetrachloride = 357.75 g / 225 cm^3 ≈ 1.59 g/cm^3. Consequently, the density of carbon tetrachloride is approximately 1.59 g/cm^3.