Chemistry, 27.08.2019 17:30 arlettehl1011

How many grams of iron (density = 7.87 g/ml ) would occupy the same volume as 96.4 g of aluminum (density = 2.70 g/ml)?

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Answer from: prettygirl1053473

280.9881 grams of iron.

Explanation:

In order to solve this we first have to calculate the volume of the aluminium because it is the one that we have all of the information to calculate:

Remember that the formula for density is:

$Density=\frac{mass}{volume}$

We clear it for volume and the result is:

$Volume=\frac{Mass}{Density}$

Now we just insert the values:

$Volume=\frac{Mass}{Density}\\Volume=\frac{96,4g}{2,7}\\Volume= 35,70ml$

Now that we have the volume we calculate how many grams of iron we need to occupy that volume, solving the formula for mas:

$Volume=\frac{Mass}{Density}\\Mass=Volume*Density\\Mass= 35,70ml*7.87g/ml\\Mass=280.9881 ml$

So the mass of iron needed to cover the same volume as 96.4 g of aluminium would be 280.9881 grams

Answer from: Quest

the answer is c. nacl

Answer from: Quest

the missing options are :

(1) lower boiling point and a lower freezing point(2) lower boiling point and a higher freezing point(3) higher boiling point and a lower freezing point(4) higher boiling point and a higher freezing point

answer : the correct answer is option (3) higher boiling point and a lower freezing point

explanation :

when a non volatile solute is added to a solvent like water, it results in elevation of boiling point.

let us find the increase in boiling point of water when cacl₂ is added to water to make a solution of 1 m

step 1 : find molality of the solution

let us assume we have 1 l of solution.

$m = \frac{moles (solute)}{l ( solution)}$

$1 m = \frac{moles (cacl_{2})}{1 l }= 1 mol cacl_{2}$

let us convert this to grams of cacl₂.

molar mass of cacl2 is 111 g/mol

grams of cacl₂ = $1 mol \times \frac{111g}{mol} = 111 g cacl_{2}$

mass of solute = 111 g

assuming density of solution same as water which is 1g/ml we have ,

mass of solution = density * volume

mass of solution = $\frac{1g}{ml} \times 1000 ml = 1000 g$

mass of solution = mass of solvent + mass of solute

mass of solute = 1000g - 111g

mass of solute 889 g = 0.889 kg

the molality of the solution can be calculated as

$molality = \frac{mol (solute)}{kg ( solvent)}$

$molality = \frac{1mol}{0.889kg}$

molality = 1.12 m

step 2 : find boiling point elevation.

the elevation in boiling point is calculated as

$\bigtriangleup t_{b} = i \times k_{b} \times m$

here δtb = boiling point elevation

i = vant hoff factor which is the number of ions formed by the solute .

cacl₂ dissociates as $cacl_{2} \rightarrow ca^{2+} + 2 cl^{-}$

it forms 3 ions . therefore,

i = 3

m = molality which is 1.12 m

kb is constant for a given solvent. for water it is 0.512

$\bigtriangleup t_{b} = 3 \times 0.512 \times 1.12$

$\bigtriangleup t_{b} = 1.7$

the boiling point of water increases by 1.7 °c

step 3: find freezing point depression.

when a non volatile solute is added to water, it results in decrease in freezing point.

the formula to find freezing point depression is

$\bigtriangleup t_{f} = i \times k_{f} \times m$

kf is constant for water and its value is 1.86

$\bigtriangleup t_{f} = 3 \times 1.86 \times 1.12$

$\bigtriangleup t_{f} = 6.2$

the freezing point of water decreases by 6.2 °c

therefore we can say that, the solution will have a higher boiling point and a lower freezing point

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How many grams of iron (density = 7.87 g/ml ) would occupy the same volume as 96.4 g of aluminum (density = 2.70 g/ml)?

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