Which gas law would apply to the following scenario.

How many atoms of oxygen does the chemical formula show?<br> Al(HSO4)3

galina1969 [7]

Answer:

This formula contains 12 oxygen atoms.

6 0

2 years ago

What is the density of a mineral with a mass of 41.2 g and a volume 8.2 cm3?

dezoksy [38]

Hey there!:

mass = 41.2 g

Volume = 8.2 cm³

Therefore:

D = m / V

D = 41.2 / 8.2

D = 5.02 g/cm³

4 0

3 years ago

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What is the mole fraction, X, of solute and the molality, m (or b), for an aqueous solution that is 15.0% NaOH by mass?

GalinKa [24]

Hello!

a) The mole fraction of solute of a 15% NaOH aqueous solution can be calculated in the following way:

First, we have to assume that we have 100 grams of solution. This will simplify the calculations.

Now, we know that this solution has 15 grams of NaOH and 85 grams of water. We can calculate the number of moles of each one in the following way:

$molesNaOH= 15 g NaOH*\frac{1molNaOH}{39,997 g NaOH}=0,3750 moles NaOH \\ \\ moles H_2O=85 gH_2O* \frac{1 mol H_2O}{18 g H_2O}=4,7222 moles H_2O$

To finish, we calculate the mole fraction by dividing the moles of NaOH between the total moles:

$X_{NaOH}= \frac{moles NaOH}{total moles}= \frac{0,3750 moles NaOH}{0,3750 moles NaOH+4,7222 molesH_2O} =0,073$

So, the mole fraction of NaOH is 0,073

b) The molality (moles NaOH/ kg of solvent) of a 15% NaOH aqueous solution can be calculated in the following way:

First, we have to assume that we have 100 grams of solution. This will simplify the calculations.

Now, we know that this solution has 15 grams of NaOH and 85 grams (0,085 kg) of water. We can calculate the moles of NaOH in the following way:

$molesNaOH= 15 g NaOH*\frac{1molNaOH}{39,997 g NaOH}=0,3750 moles NaOH$

Now, we apply the definition of molality to calculate the molality of the solution:

$mNaOH= \frac{moles NaOH}{kg_{solvent}}= \frac{0,3750 moles NaOH}{0,085 kg H_2O}=4,41 m$

So, the molality of this solution is 4,41 m

Have a nice day!

4 0

3 years ago

if I add water to 170 mL of a 0.40 M KOH solution until the final volume is 375 mL, what will the molarity M of the diluted solu

nasty-shy [4]

4.7 M It may be wrong, but I hope it helps!

Explanation:

When you're diluting a solution, you're essentially keeping the number of moles of solute constant while changing the total volume of the solution.

Now, let's assume that you don't know the equation for dilution calculations.

In this case, you can use the molarity and volume of the concentrated solution to determine how many moles of hydrochloric acid you start with.

c

=

n

V

⇒

n

=

c

⋅

V

n

HCl

=

18 M

⋅

190

⋅

10

−

3

L

=

3.42 moles HCl

You then add water to get the total volume of the solution from

190 mL

to

730 mL

.

The number of moles of hydrochloric acid remains unchanged, which means that the molarity of the diluted solution will be

c

=

3.42 moles

730

⋅

10

−

3

L

=

4.7 M

8 0

2 years ago

A hypothesis must be testable and falsifiable to be considered scientific

Zarrin [17]

Its TRUE because the hypothesis is only true when you have facts behind it has to be testable

7 0

3 years ago

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