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3 years ago

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A chemist adds of a aluminum chloride solution to a flask. Calculate the mass in grams of aluminum chloride the chemist has adde

d to the flask. Be sure your answer has the correct number of significant digits.

1 answer:

DerKrebs [107]3 years ago

4 0

The given question is incomplete. The complete question is:

A chemist adds 95.0 ml of a 1.5M aluminum chloride solution to a flask. Calculate the mass in grams of aluminum chloride the chemist has added to the flask. Be sure your answer has the correct number of significant digits.

Answer: 19.0 grams

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

$Molarity=\frac{n\times 1000}{V_s}$

where,

n = moles of solute

$V_s$ = volume of solution in ml

moles of $AlCl_3$ = $\frac{\text {given mass}}{\text {Molar mass}}=\frac{xg}{133.34g/mol}$

Now put all the given values in the formula of molarity, we get

$1.5=\frac{x\times 1000}{95.0\times 133.34}$

$x=19.0g$

Therefore, the mass in grams of aluminum chloride the chemist has added to the flask is 19.0

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How many molecules in 9.18 moles of C11H12O22

Setler [38]

Answer:

55.3 × 10²³ molecules

Explanation:

Given data:

Number of moles of C₁₁H₁₂O₂₂ = 9.18 mol

Number of molecules = ?

Solution:

The given problem will solve by using Avogadro number.

It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance.

The number 6.022 × 10²³ is called Avogadro number.

For example,

18 g of water = 1 mole = 6.022 × 10²³ molecules of water

For given data:

9.18 mol × 6.022 × 10²³ molecules /1 mol

55.3 × 10²³ molecules

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3 years ago

In solid NaCl, the equilibrium separation between neighboring Na+ and Cl- ions is 0.283 nm. Calculate the coulombic energy betwe

const2013 [10]

Explanation:

It is given that r = 0.283 nm. As 1 nm = $10^{-9} m$ .

Hence, 0.283 nm = $0.283 \times 10^{-9} m$

Formula for coulombic energy is as follows.

$U_{coulomb} = -1.748 \frac{e^{2}}{4 \pi \epsilon_{o} r}$

where, e = $1.6 \times 10^{-19}$ C

$\epsilon_{o}$ = $8.85 \times 10^{-12}$

$U_{coulomb} = -1.748 \frac{(1.6 \times 10^{-19}^{2}}{4 \times 3.14 \times 8.85 \times 10^{-12} \times 0.283 \times 10^{-9}}$

= $1.423 \times 10^{-18} J$

As 1 eV = $1.6 \times 10^{-19} J$

So, 1 J = $\frac{1 eV}{1.6 \times 10^{-19}}$

Hence, U = $\frac{1.423 \times 10^{-18} J}{1.6 \times 10^{-19} J}$

= 8.9 eV

Also, 1 J = $\frac{10^{-3} kJ}{6.022 \times 10^{23}mol}$

= $1.67 \times 10^{-27}$ kJ/mol

Therefore, U = $1.423 \times 10^{-18} J \times 1.67 \times 10^{-27}$ kJ/mol

= $2.37 \times 10^{-45} kJ/mol$

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3 years ago

A sample of gas occupies a volume of 10.5 L when the pressure is 14.3 psi. Use Boyle’s Law to calculate the pressure (psi) when

Nutka1998 [239]

Answer: 17.6psi

Explanation:

V1 = 10.5 L

P1 = 14.3 psi

V2 = 8.55L

P2 =?

P1V1 = P2V2

14.3 x 10.5 = P2 x 8.55

P2 = (14.3 x 10.5) / 8.55

P2 = 17.6psi

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3 years ago

Read 2 more answers

The electron-domain geometry of a carbon-centered compound ch4 is tetrahedral. the hybridization of the central carbon atom is _

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The hybridization of the central carbon compound CH4 tetrahedral is
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3 years ago

The forensic technician at a crime scene has just prepared a luminol stock solution by adding 16.0 g of luminol into a total vol

nikitadnepr [17]

The molarity of the stock solution of luminol is 1.2 M

<u><em>calculation</em></u>

step 1: find the moles of luminol using (moles= mass/molar mass) formula

molar mass of Luminol= 177 g/mol

moles is therefore= 16.0 g/ 177 g/mol=0.0904 moles

Step 2: find the molarity using (molarity= moles/volume in liters) formula

convert Ml into liters = 75.0/1000= 0.075 L

molarity is therefore= 0.0904 moles/ 0.075 L= 1.2M

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3 years ago