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spin [16.1K]
3 years ago
13

Ethanol has a density of 0.789 g/cm3. What is the mass of 423 cm3 of ethanol? M = (D)(V)

Chemistry
1 answer:
Ivahew [28]3 years ago
6 0

Answer:

<h2>The answer is 334 g</h2>

Explanation:

The mass of a substance when given the density and volume can be found by using the formula

<h3>mass = Density × volume</h3>

From the question

volume of ethanol = 423 cm³

density = 0.789 g/cm³

So we have

mass = 0.789 × 423 = 333.747

We have the final answer as

<h3>334 g</h3>

Hope this helps you

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BY The Editors of Encyclopaedia Britannica | View Edit History

ion, any atom or group of atoms that bears one or more positive or negative electrical charges. Positively charged ions are called cations; negatively charged ions, anions. Ions are formed by the addition of electrons to, or the removal of electrons from, neutral atoms or molecules or other ions; by combination of ions with other particles; or by rupture of a covalent bond between two atoms in such a way that both of the electrons of the bond are left in association with one of the formerly bonded atoms. Examples of these processes include the reaction of a sodium atom with a chlorine atom to form a sodium cation and a chloride anion; the addition of a hydrogen cation to an ammonia molecule to form an ammonium cation; and the dissociation of a water molecule to form a hydrogen cation and a hydroxide anion.

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2 years ago
What is the normal ph of rain?
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3 years ago
A mixture of krypton and argon gases, at a total pressure of 733 mm Hg, contains 3.97 grams of krypton and 6.34 grams of argon.
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Answer:

Partial pressure of krypton= 167.12 mmHg

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Explanation:

The partial pressure of a gas in a mixture of gasses is equal to the total pressure multiplied (Pt) by the mole fraction of the gas (X):

P= X Pt

The total pressure is Pt= 733 mmHg

The mole fraction is given by the following:

X = number of moles of gas/ total number of moles

For krypton (Kr) , the molecular weight is 83.8 g/mol and we calculate the number of moles by dividing the mass into the molecular weight as follows:

moles of Kr = 3.97 g/(83.8 g/mol)= 0.047 moles

For argon (Ar), the molesular weight is 39.9 g/mol, so we calculate the number of moles as follows:

moles of Ar = 6.34 g/(39.9 g/mol)= 0.159

Now, we calculate the total number of moles (nt):

nt= moles of Kr + moles of Ar = 0.047 moles + 0.159 moles = 0.206 moles

The mole fraction of each gas is now calculated:

X(Kr)= moles of Kr/nt = 0.047 moles/0.206 = 0.228

X(Ar)= moles of Ar/nt = 0.159 moles/0.206 = 0.772

Finally, with the mole fractions and the total pressure we calculate the partial pressure of each gas as follows:

P(Kr) = X(Kr) x Pt = 0.228 x 733 mmHg= 167.12 mmHg

P(Ar) = X(Ar) x Pt = 0.772 x 733 mmHg= 565.88 mmHg

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