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3 years ago

A compound contains 75% carbon and 25% hydrogen by mass. What is the empirical formula for this compound?

Chemistry

2 answers:

lubasha [3.4K]3 years ago

7 0

Answer: The empirical formula for this compound is CH4

Explanation:

timama [110]3 years ago

6 0

The empirical formula would be CH4.

“To get the empirical formula of the compound, we convert each mass percentage to mole percentage by dividing each to corresponding molar mass. 75% mass of carbon is 6.25 while 25% hydrogen is 25. We divide 25 by 6.25, we get 4. Hence, the empirical formula is CH4.”

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Magnets are classified based upon how they occur either naturally or man made true or false

slega [8]

Answer:

True

Explanation:

Permanent artificial, temporary artificial and natural. They are classified by the way in which they have achieved magnetism and by how long they remain magnetic.

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3 years ago

An atom has 5 neutrons,2electrons and 4 protons what type of atom is it

satela [25.4K]

Answer:

Cation

Explanation:

Since the protons are greater than electrons, this means the atom has a net positive charge on it and is now called a cation.

As there are 4 protons, this means that the outermost shell has 2 valence electrons 2s1, 2s2 and this is Group 2 element. Looking at Periodic table, we find that this is beryllium 4Be5 and is denoted as Be^2+

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3 years ago

Photosynthesis produces

dmitriy555 [2]

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3 years ago

How many grams of zinc metal will react completely with 7.8 liters of 1.6 M HCl? Show all of the work needed to solve this probl

Andru [333]

Answer:

For 1: The correct answer is 407.97 grams.

For 2: The correct answer is 76.72 grams.

Explanation:

For 1:

We are given the molarity of HCl, to find the moles of HCl, we use the formula:

$Molarity=\frac{\text{Moles}{\text{Volume}}$

We are given:

Molarity = 1.6 M

Volume = 7.8 L

Putting values in above equation, we get:

$1.6mol/L=\frac{\text{Moles of HCl}}{7.8L}\\\\\text{Moles of HCl}=12.48mol$

For the given reaction:

$Zn(s)+2HCl(aq.)\rightarrow ZnCl_2(aq.)+H_2(g)$

By Stoichiometry of the reaction:

2 moles of HCl reacts with 1 mole of zinc metal.

So, 12.48 moles of HCl react with = $\frac{1}{2}\times 12.48=6.24mol$ of Zinc metal.

To calculate the mass of zinc metal, we use the formula:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Molar mass of Zinc metal = 65.38 g/mol

$6.24=\frac{\text{Mass of zinc metal}}{65.38g/mol}\\\\\text{Mass of zinc metal}=407.97g$

For 2:

We are given that 298 grams of 83.1 % by mass of iron (II) nitrate solution are present.

So, mass of Iron (II) nitrate solution will be = $\frac{83.1}{100}\times 298=247.638g$

Molar mass Iron (II) nitrate = 180 g/mol

Putting values in equation 1, we get:

$\text{Moles of }Fe(NO_3)_2=\frac{247.638g}{180g/mol}=1.37mol$

For the following reaction:

$2Al(s)+3Fe(NO_3)_2(aq.)\rightarrow 3Fe(s)+2Al(NO_3)_3(aq.)$

By Stoichiometry of the reaction:

3 moles of $Fe(NO_3)_2$ produces 3 moles of iron metal.

So, 1.37 moles of $Fe(NO_3)_2$ will produce = $\frac{3}{3}\times 1.37=1.37mol$ of iron metal.

To calculate the mass of zinc metal, we equation 1:

$1.37=\frac{\text{Mass of iron metal}}{56g/mol}\\\\\text{Mass of iron metal}=76.72g$

5 0

3 years ago

SOMEONE PLEASE HELP ME ASAP PLEASE!!!!!

Afina-wow [57]

Answer:

P₂ = 592.7 torr

Explanation:

Given data:

Initial Pressure = 215 torr

Initial volume = 51.0 mL

Final pressure = ?

Final volume = 18.5 mL

Solution:

P₁V₁ = P₂V₂

P₁ = Initial Pressure

V₁ = Initial volume

P₂ = Final pressure

V₂ = Final volume

Now we will put the values in formula.

P₁V₁ = P₂V₂

215 torr × 51.0 mL = P₂ × 18.5 mL

10965 mL. torr = P₂ × 18.5 mL

P₂ = 10965 mL. torr /18.5 mL

P₂ = 592.7 torr

8 0

3 years ago