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3 years ago

How many molecules are in 4.5 moles of H2O?

Chemistry

1 answer:

Evgen [1.6K]3 years ago

6 0

Answer:

There would be around 2.7*10^24 molecules.

Explanation:

You have to multiply the amount of moles by Avogadro's number to get amount of molecules.

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What is the density of carbon dioxide gas if 0.196g occupies a volume of 100mL?

-BARSIC- [3]

We know that the equation for density is:

$D=\frac{m}{V}$

where D is the density, m is the mass in grams, and V is the volume.

Given two of the variables, we can then solve for density:

$D=\frac{0.196g}{100mL}= \frac{0.00196g}{mL}$

So therefore, we now know that the density of carbon dioxide gas is 0.00196g/mL.

7 0

3 years ago

In the following equation:

Luda [366]

Answer:

FeCl₃

Explanation:

4FeCl₃ + 3O₂ => 2Fe₂O₃+ 6Cl₂

Given => 7moles 9moles

A simple way to determine which reagent is the limiting reactant is to convert all given data to moles then divide by the respective coefficients of the balanced equation. The smaller value will be the limiting reactant.

4FeCl₃ + 3O₂ => 2Fe₂O₃+ 6Cl₂

Given => 7/4 = 1.75* 9/3 = 3

*Smaller value => FeCl₃ is limiting reactant.

NOTE: However, when working problems, one must use original mole values given.

7 0

3 years ago

Which base has the lowest ionization constant (Kb)?

inysia [295]

Answer:D.Blood

Explanation:

4 0

3 years ago

Look at sample problem 19.10 in the 8th ed Silberberg book. Write the Ksp expression. Find the concentrations of the ions you ne

777dan777 [17]

Answer:

Explanation:

From the information given:

$CaF_2 \to Ca^{2+} + 2F^-$

$Ksp = 3.2 \times 10^{-11}$

no of moles of $Ca^{2+}$ = 0.01 L × 0.0010 mol/L

no of moles of $Ca^{2+}$ = $1 \times 10^{-5} \ mol$

no of moles of $F^-$ = 0.01 L × 0.00010 mol/L

no of moles of $F^-$ = $1 \times 10^{-6}\ mol$

Total volume = 0.02 L

$[Ca^{2+}}] = \dfrac{1\times10^{-5} \ mol}{0.02 \ L} \\ \\ \\ \[[Ca^{2+}}] = 0.0005 \ mol/L$

$[F^{-}] = \dfrac{(1\times 10^{-6} \ mol)}{0.02 \ L}$

$[F^{-}] = 5 \times 10^{-5} \ mol/L$

$Q = [Ca^{2+}][F^-]^2 \\ \\ Q = 0.0005 \times (5\times 10^{-5})^2 \\ \\ Q = 1.25 \times 10^{-12}$

Since Q<ksp, then there will no be any precipitation of CaF2

3 0

3 years ago

Pls help asap!!!!

AVprozaik [17]

Answer: The pressure of the He is 2.97 atm

Explanation:

According to Dalton's law, the total pressure is the sum of individual pressures.

$p_{total}=p_{N_2}+p_{O_2}+p_{He}.$

Given : $p_{total}$ =total pressure of gases = 6.50 atm

$p_{N_2}$ = partial pressure of Nitrogen = 1.23 atm

$p_{O_2}$ = partial pressure of oxygen = 2.3 atm

$p_{He}$ = partial pressure of Helium = ?

putting in the values we get:

$6.50atm=1.23atm+2.3atm+p_{He}$

$p_{He}=2.97atm$

The pressure of the He is 2.97 atm

3 0

3 years ago