All categories

3 years ago

If a sample of 0.362 m lithium phosphate contains 0.284 g of lithium, what is the volume of the sample?

Chemistry

2 answers:

Leni [432]3 years ago

7 0

Answer;

= 0.03791 Liters

Solution and explanation;

-The molar mass of Li3PO4 is 115.79 g/mol.

-If lithium is 6.9 g/mol, multiplied by 3 (from Li3PO4), that would be 20.7 g/mol.

-Now we can use this to find the percentage of Li in Li3PO4, 20.7/115.79 = 0.1788 or 17.88%

-This 17.88% can tell us the mass of Li3PO4 using the mass which 0.284. Now lets divide 0.284 by 0.1788 = 1.589 g. This now the mass of Li3PO4.

-Using that, we can now easily find the moles of Li3PO4,

using the molar mass. So (1.589g)(1mol/115.79g)=0.013723 moles of Li3PO4.

-From this, we can now find the volume using molarity (0.362), which is moles per Liter.

= (0.013723 moles)(1L/0.362mol)=0.03791 L

fenix001 [56]3 years ago

3 0

From the periodic table:
mass of lithium = 6.941 grams
number of moles = mass / molar mass
number of moles of Li = 0.284 / 6.941 = 0.0409 moles

Molarity can be calculated using the following rule:
molarity = number of moles of solute / liters of solution
volume (in liters) = number of moles of solute / molarity
volume = 0.0409 / 0.362 = 0.1129 liters

You might be interested in

The table shows the average sleeping time of different organisms. According to the table above, the amount of sleep needed by hu

artcher [175]

Reduces from birth till old age is the answer because if you look at the chart, you can see that both the percentages and hours of total sleep time decrease as humans get older.

7 0

3 years ago

When a 1.06 g sample of Compound Q, a nonelectrolyte, is dissolved in 11.6 g of water, the boiling point of the resulting soluti

Vesna [10]

Answer:

The molar mass of compound Q is 100 g/mol

Explanation:

Step 1: Data given

Mass of compound Q = 1.06 grams

Mass of water = 11.6 grams

Boiling point of the solution = 100.47 °C

Boiling point of water = 100.00 °C

Kb for water = 0.512 °C/m

Step 2: Calculate molality

ΔT = i*kb*m

⇒ with ΔT = the boiling point elevation = 0.47 °C

⇒ with i = the van't Hoff factor = 1

⇒ with kb = the boiling point elevation constant = 0.512 °C/m

⇒ with m = the molality = moles compound Q / mass water

m = ΔT / (i*Kb)

m = 0.47 / 0.512

m = 0.918 molal

Step 3: Calculate moles of Q

Molality = moles Q / mass H2O

moles Q = 0.918 molal * 0.0116 kg

moles Q = 0.0106 moles

Step 4: Calculate molar mass

Molar mass Q = mass Q / moles Q

Molar mass Q = 1.06 grams / 0.0106 moles

Molar mass Q = 100 g/mol

The molar mass of compound Q is 100 g/mol

3 0

3 years ago

Epirical formula of P4O10

harina [27]

I would say the answer is P2O5. Some teachers use PO2.5. I'm not one of them.

7 0

4 years ago

5.98 g of K Al(SO4)2 is equivalent to how many moles?

Rasek [7]

Answer:

Molecular Weight Of KAl(SO4)2 12H2O = 475 G / Mol Molecular Weight Of Al = 27 G / Moles.

Explanation:

HOPE THIS HELPS YOU OUT AND IF IT DID PLS MARK ME AS BRAINIEST

4 0

3 years ago

If a solution containing 51.429 g of mercury(ii) perchlorate is allowed to react completely with a solution containing 16.642 g

OLga [1]

Hg(No3)2 +NaSO4 --->2NaNO3 + HgSO4(s)
calculate the moles of each reactant
moles=mass/molar mass

moles of Hg(NO3)2= 51.429g/ 324.6 g/mol(molar mass of Hg(NO3)2)=0.158 moles

moles Na2SO4 16.642g/142g/mol= 0.117 moles of Na2SO4

Na2SO4 is the limiting reagent in the equation and by use mole ratio Na2So4 to HgSO4 is 1:1 therefore the moles of HgSO4 =0.117 moles

mass of HgSO4=moles x molar mass of HgSo4= 0.117 g x 303.6g/mol= 35.5212 grams

7 0

4 years ago