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Allisa [31]
3 years ago
10

22. A cubic object has sides with lengths of 6.0 cm,

Chemistry
2 answers:
fiasKO [112]3 years ago
5 0

Answer : The correct option is, (3) 4.5g/cm^3

Explanation :

Density : It is defined as the mass contained per unit volume.

Formula used :

Density=\frac{Mass}{Volume}

First we have to calculate the volume of cuboid.

Formula used :

V=l\times b\times h

where,

V = volume of cuboid

l = length of cuboid = 6.0 cm

b = breadth of cuboid = 3.0 cm

h = height of cuboid = 2.0 cm

Now put all the given values in the above formula, we get:

V=6.0cm\times 3.0cm\times 2.0cm=36cm^3

Now we have to calculate the density of cube.

Given :

Mass of cube = 162.2 g

Volume of cube = 36cm^3

Now put all the given values in the above formula, we get :

Density=\frac{162.2g}{36cm^3}=4.5g/cm^3

Therefore, the density of cube is 4.5g/cm^3

eduard3 years ago
3 0

Answer:

option 4 =4.505 g/cm³

Explanation:

Density:

Density is equal to the mass of substance divided by its volume.

Units:

SI unit of density is Kg/m3.

Other units are given below,

g/cm3, g/mL , kg/L

Formula:

D=m/v

D= density

m=mass

V=volume

Symbol:

The symbol used for density is called rho. It is represented by ρ. However letter D can also be used to represent the density.

Given data:

Mass of cube = 162.2 g

density = ?

Volume =  6cm× 3cm×2cm = 36cm³

Solution:

d= m/v

d = 162.2 g/ 36 cm³

d = 4.505 g/cm³

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The molar mass is determined by measuring the freezing point depression of an aqueous solution. A freezing point of -5.20°C is r
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Answer:

The empirical formula is C2H4O3

The molecular formula is C4H8O6

The molar mass is 152 g/mol

Explanation:

The complete question is: An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound gives mass percents of 31.57% C and 5.30% H. The molar mass is determined by measuring the freezing-point depression of an aqueous solution. A freezing point of -5.20°C is recorded for a solution made by dissolving 10.56 g of the compound in 25.0 g water. Determine the empirical formula, molar mass, and molecular formula of the compound. Assume that the compound is a nonelectrolyte.

Step 1: Data given

Mass % of Carbon = 31.57 %

Mass % of H = 5.30 %

Freezing point = -5.20 °C

10.56 grams of the compound dissolved in 25.0 grams of water

Kf water = 1.86 °C kg/mol

Step 2: Calculate moles of Carbon

Suppose 31.57% = 31.57 grams

moles C = mass C / Molar mass C

moles C = 31.57 grams / 12.0 g/mol = 2.63 moles

Step 3: Calculate moles of Hydrogen:

Moles H = 5.30 grams / 1.01 g/mol

moles H = 5.25 moles

Step 4: Calculate moles of Oxygen

Moles O = ( 100 - 31.57 - 5.30) / 16 g/mol

Moles O = 3.95 moles

Step 5: We divide by the smallest number of moles

C: 2.63 / 2.63 = 1 → 2

H: 5.25/2.63 = 2 → 4

O: 3.95/ 2.63 = 1.5 → 3

The empirical formula is C2H4O3

The molar mass of the empirical formula = 76 g/mol

Step 6: Calculate moles solute

Freezing point depression = 5.20 °C = m * 1.86

m = 5.20 / 1.86

m = 2.80 molal = 2.80 moles / kg

2.80 molal * 0.025 kg = 0.07 moles

Step 7: Calculate molar mass

Molar mass = mass / moles

Molar mass = 10.56 grams / 0.07 moles

Molar mass = 151 g/mol

Step 8: Calculate molecular formula

151 / 76 ≈  2

We have to multiply the empirical formula by 2

2*(C2H4O3) = C4H8O6

The molecular formula is C4H8O6

The molar mass is 152 g/mol

6 0
4 years ago
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