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Airida [17]
3 years ago
10

An unknown compound is found to have a molar mass of 392.16 g/mol. If the empirical formula is C2H5PF2, what is the molecular fo

rmula
Chemistry
1 answer:
notsponge [240]3 years ago
8 0

Answer:

C8H20P4F8

Explanation:

Molecular formula is based off a ratio of the molecular formula's molar mass divided by the empirical formula's molar mass.

The molar mass of the empirical formula C2H5PF2 is 98.02g. We find this by adding the molar masses of all elements in the formula, multiplied by their subscripts.

2(12.01) + 5(1.01) + 30.97 + 2(18.99) = 98.02

We then divide the molecular molar mass by the empirical molar mass.

392.16/98.02 = 4

This tells us that the molecular formula has 4 times the mass of the empirical formula. Because mass comes from the elements in the formula, we multiply all the subscripts by 4 to get the molecular formula.

2x4 = 8

5x4 = 20

1x4 = 4

2x4 = 8

So the molecular formula is C8H20P4F8

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What is the percent composition of calcium fluoride
vladimir1956 [14]

Answer:

78.07

Explanation:

them seperatly is

Calcium Ca 51.333%

Fluorine F 48.667%

8 0
2 years ago
What is the empirical formula
lord [1]

A formula giving the proportions of the elements present in a compound but not the actual numbers or arrangement of atoms.

5 0
3 years ago
A sample of juice has a pH of 4.2. Whsat is the concentration in mol/dm3 of OH in the juice?<br>​
Annette [7]

Answer:

6 * 10^-4M

Explanation:

use this equation

[ H + ]  =  10  −  pH

6 0
3 years ago
Using the following thermochemical equation, determine the amount of heat produced per kg of CO2 formed during the combustion of
Arisa [49]

Answer:  12033 kJ of heat produced per kg of CO_2 formed during the combustion of benzene

Explanation:

The balanced chemical equation for combustion of benzene is :

2C_6H_6(l)+15O_2(g)\rightarrow 12CO_2(g)+6H_2O(g)  \Delta H°rxn = -6278 kJ

Exothermic reactions are defined as the reactions in which energy of the product is lesser than the energy of the reactants. The total energy is released in the form of heat and \Delta H for the reaction comes out to be negative.

\text{Moles of }CO_2=\frac{\text{given mass}}{\text{Molar Mass}}=\frac{1000g}{44g/mol}=23mol      (1kg=1000g)

According to stoichiometry :

12 moles of CO_2 on combustion produce heat = 6278 kJ

Thus 23 mole of CO_2 on combustion produce heat =\frac{6278}{12}\times 23=12033kJ

Thus 12033 kJ of heat produced per kg of CO_2 formed during the combustion of benzene

5 0
3 years ago
Which aqueous solution of KI freezes at the lowest temperature?
slavikrds [6]

Answer:

b. 2 mol of KI in 500. g of water

Explanation:

We have to apply the colligative property of freezing point depression.

The formula is: ΔT = Kf . m . i

As the (Kf . m . i) is higher, then the freezing temperature will be lower.

i refers to the Van't Hoff factor (number of ions dissolved in the solution)

KI → K⁺ + I⁻    (i =2)

Kf is constant so, we have to search for the highest m (molality)

Molality means the moles of solute in 1kg of solvent.

The highest m is option b → 2 mol of KI / 0.5 kg = 4 mol/kg

a. 1 mol of KI / 0.5 kg = 2 mol/kg

c. 1 mol of KI / 1kg = 1 mol/kg

d. 2 mol of KI / 1kg = 2 mol/kg

1000 g = 1kg. In order to determine molality we need to convert the mass (g) of solvent to kg

3 0
3 years ago
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