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4 years ago

* Need ASAP * Explain the relationship between percent composition, Empirical formula, and molecular formula.

1 answer:

5 0

By dividing the percentage composition with the molar mass of that element we will get the empirical formula. Then using that empirical formula and formula mass we can find the molecular formula.

Explanation:

The chemical properties of any substance are defined obviously by the different types and relative amounts of atoms constituting its primary entities (in case of covalent compounds the primary entities are molecules and ions in the event of ionic compounds).

A percent composition of any compound gives the mass percent of each element present in the compound; in addition to that frequently it is determined experimentally and utilized to derive an empirical formula of any compound. An empirical formula mass of any covalent compound could be comparable with the molar or molecular mass of a compound to acquire a molecular formula.

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3 years ago

Calculate the ratio of effusion rates for helium and argon.

lys-0071 [83]

Answer : The ratio of effusion rates for helium and argon is 3.2 : 1

Solution : Given,

Molar mass of Helium = 4 g/mole

Molar mass of Argon = 40 g/mole

Rate of effusion : It is defined as the rate of effusion of a gas is inversely proportional to the square root of the molar mass of the gas.

Formula used :

$\text{Rate of effusion}=\frac{1}{\sqrt{M}}$

where, M is the molar mass.

$\frac{Rate_{He}}{Rate_{Ar}}=\sqrt{\frac{M_{Ar}}{M_{He}}}$

Now put all the given values in this expression, we get

$\frac{Rate_{He}}{Rate_{Ar}}=\sqrt{\frac{40}{4}}=\frac{3.2}{1}$

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3 years ago

At the _______ point of a substance, the particles have enough kinetic energy to break free from their fixed positions.

Natasha_Volkova [10]

Answer:

At the nucleus point of a substance, the particles have enough kinetic energy to break free from their fixed positions.

Answer : nucleus

5 0

2 years ago

Calculate the mass of each product formed when 84.3 g of silver sulfide reacts with excess hydrochloric acid: ag2s(s) + hcl(aq)

oee [108]

Answer:

48.75 g of AgCl

11.60 g of H₂S

Solution:

The Balance Chemical Equation is as follow,

Ag₂S + HCl → AgCl + H₂S

Calculate amount of AgCl produced,

According to equation,

247.8 g (1 mol) of Ag₂S produces = 143.32 g (1 mol) of AgCl

So,

84.3 g of Ag₂S will produce = X g of AgCl

Solving for X,

X = (84.3 g × 143.32 g) ÷ 247.8 g

X = 48.75 g of AgCl

Calculate amount of H₂S produced,

According to equation,

247.8 g (1 mol) of Ag₂S produces = 34.1 g (1 mol) of H₂S

So,

84.3 g of Ag₂S will produce = X g of H₂S

Solving for X,

X = (84.3 g × 34.1 g) ÷ 247.8 g

X = 11.60 g of H₂S

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3 years ago

At what temperature is the volume of the gas 4.00 L if the pressure is kept constant.

marta [7]

Its B

Explanation:

Thats should help you out

3 0

3 years ago