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2 years ago

A 23.0g sample of a compound contains 12.0g of C, 3.0g of H, and 8.0g of O.What the empirical formula of the compound

Chemistry

1 answer:

Kryger [21]2 years ago

5 0

Answer:

The empirical formula of compound is C₂H₆O.

Explanation:

Given data:

Mass of carbon = 12 g

Mass of hydrogen = 3 g

Mass of oxygen = 8 g

Empirical formula of compound = ?

Solution:

First of all we will calculate the gram atom of each elements.

no of gram atom of carbon = 12 g / 12 g/mol = 1 g atoms

no of gram atom of hydrogen = 3 g / 1 g/mol = 3 g atoms

no of gram atom of oxygen = 8 g / 16 g/mol = 0.5 g atoms

Now we will calculate the atomic ratio by dividing the gram atoms with the 0.5 because it is the smallest number among these three.

C:H:O = 1/0.5 : 3/0.5 : 0.5/0.5

C:H:O = 2 : 6 : 1

The empirical formula of compound will be C₂H₆O

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The answer is bohr hope this helps :)

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1 year ago

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If 89.6 joules of heat are needed to heat 20.0 grams of iron from 30.0°c to 40.0°c, what is the specific heat of the iron in jg?

klasskru [66]

The relation of heat (Q), mass (m), and change of temperature (ΔT) is given by the formula:

Q = m*Cs*ΔT, where Cs is the specific heat of the material.

Then, given than you know Q, m and ΔT, you can solv for Cs:

Cs = Q / (m*ΔT)

Cs = 89.6 J / [20 grams * (40.0°C - 30.0°C)] = 0.448 J / g * °C.

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2 years ago

A 3.96x10^-24 M solution of compound A exhibited an absorbance of 0.624 at 238 nm in a 1.000-cm cuvet; a blank solution containi

viktelen [127]

Actual question from source:-

A 3.96x10-4 M solution of compound A exhibited an absorbance of 0.624 at 238 nm in a 1.000 cm cuvette. A blank had an absorbance of 0.029. The absorbance of an unknown solution of compound A was 0.375. Find the concentration of A in the unknown.

Answer:

Molar absorptivity of compound A = $1502.53\ {Ms}^{-1}$

Explanation:

According to the Lambert's Beer law:-

$A=\epsilon l c$

Where, A is the absorbance

l is the path length

$\epsilon$ is the molar absorptivity

c is the concentration.

Given that:-

c = $3.96\times 10^{-4}\ M$

Path length = 1.000 cm

Absorbance observed = 0.624

Absorbance blank = 0.029

A = 0.624 - 0.029 = 0.595

So, applying the values in the Lambert Beer's law as shown below:-

$0.595=\epsilon\times 1.000\ cm\times 3.96\times 10^{-4}\ M$

$\epsilon=\frac{0.595}{3.96\times 10^{-4}}\ {Ms}^{-1}=1502.53\ {Ms}^{-1}$

<u>Molar absorptivity of compound A = $1502.53\ {Ms}^{-1}$ </u>

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2 years ago

Larisa pumps up a soccer ball until it has a gauge pressure of 61 kilopascals. The volume of the ball is 5.2 liters. The air tem

Nuetrik [128]

<h3>Answer:</h3>

B. 0.33 mol

<h3>Explanation:</h3>

We are given;

Gauge pressure, P = 61 kPa (but 1 atm = 101.325 kPa)

= 0.602 atm

Volume, V = 5.2 liters

Temperature, T = 32°C, but K = °C + 273.15

thus, T = 305.15 K

We are required to determine the number of moles of air.

We are going to use the concept of ideal gas equation.

According to the ideal gas equation, PV = nRT, where P is the pressure, V is the volume, R is the ideal gas constant, (0.082057 L.atm mol.K, n is the number of moles and T is the absolute temperature.

Therefore, to find the number of moles we replace the variables in the equation.
Note that the total ball pressure will be given by the sum of atmospheric pressure and the gauge
Therefore;
Total pressure = Atmospheric pressure + Gauge pressure

We know atmospheric pressure is 101.325 kPa or 1 atm

Total ball pressure = 1 atm + 0.602 atm

= 1.602 atm

That is;

PV = nRT

n = PV ÷ RT

therefore;

n = (1.602 atm× 5.2 L) ÷ (0.082057 × 305.15 K)

= 0.3326 moles

= 0.33 moles

Therefore, there are 0.33 moles of air in the ball.

4 0

2 years ago

The molar mass of an imaginary molecule is is 93.89 g/mol. Determine its density at STP.

Igoryamba

Answer:

Density = 4.191 gm/L

Explanation:

Given:

Molar mass = 93.89 g/mol

Volume(Missing) = 22.4 L (Approx)

Find:

Density at STP

Computation:

Density = Mass/Volume

Density = 93.89 / 22.4

Density = 4.191 gm/L

3 0

1 year ago