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3 years ago

What will the volume be of a soltuion created using 120 ml of 4.5 M stock solution if the final molarity needs to be 2.00 M

Chemistry

1 answer:

Troyanec [42]3 years ago

3 0

Answer:

We need 540 mmoles of stock solution and complete to 270 mL of volume.

Explanation:

In order to determine the volume or concentration at diluted solution we apply this formula:

Dil volume . Dil concentration = Conc volume . Conc concentration

Stock solution is always, the concentrated.

Let's replace with data given:

Dil. volume . 2 M = 120 mL . 4.5 M

Diluted volume = (120 mL . 4.5M) / 2M

Diluted volume = 270 mL

This problem can be also solved by rule of three:

1 mL of stock solution contains 4.5 mmoles

120 mL of stock solution contain (120 mL . 4.5 mmoles) / 1mL = 540 mmoles

This mmoles of stock solution are also contained at the diluted

If 2 mmoles are contained in 1mL of diluted solution

540 mmoles must be contained in (540 mmol . 1 mL) / 2 mmol = 270 mL

We need 540 mmoles of stock solution and complete to 270 mL of volume.

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Varvara68 [4.7K]

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3 years ago

This is what your screen should look like. start with Hydrogen -1 and drag 2 neutrons over the to the nucleus. What happens to t

Alekssandra [29.7K]

Answer:

A tritium is produced.

Explanation:

Combining two additional neutrons to the nucleus of the hydrogen atom makes it a tritium, Hydrogen-3.

neutron is designated ¹₀n; this shows a mass number of 1 and no atomic number

Hydrogen-1 is designated as ₁¹H; a mass number of 1 and atomic number of 1. This particle is actually more like a proton.

Combining both:

₁¹H + 2¹₀n → ³₁H

This is a nuclear reaction and in balancing such reaction equation, mass numbers and atomic numbers must be conserved.

4 0

3 years ago

An analysis of a sugar compound is found to contain 132 grams of carbon (C), 22 grams of hydrogen (H), and 176 grams of oxygen (

ddd [48]

132 g of C , 22 g of H , 176 g of O

132 + 22 + 176 => 330 g of the substance

Now convert the masses in moles :

C = 12.0 u H = 1.0 u O = 16.0 u

C = 132 / 12.0 => 11 moles

H = 22 / 1.0 => 22 moles

O = 176 / 16.0 => 11 moles

Using the values obtained the lowest proportion in mols of elements present, simply divide the values found for the least of them:

C = 11 / 11 => 1

H = 22 / 11 => 2

O = 11 / 11 => 1

formula empirically is : CH₂O

hope this helps!

8 0

4 years ago

Determine the mass of CaCO3 required to produce 40.0 mL CO2 at STP. Hint use molar volume of an ideal gas (22.4 L)

cupoosta [38]

Answer:

$m_{CaCO_3}=0.179gCaCO_3$

Explanation:

Hello,

In this case, since the undergoing chemical reaction is:

$CaCO_3(s)\rightarrow CaO(s)+CO_2(g)$

The corresponding moles of carbon dioxide occupying 40.0 mL (0.0400 L) are computed by using the ideal gas equation at 273.15 K and 1.00 atm (STP) as follows:

$PV=nRT\\\\n=\frac{PV}{RT}=\frac{1.00 atm*0.0400L}{0.082\frac{atm*L}{mol*K}*273.15 K})=1.79x10^{-3} mol CO_2$

Then, since the mole ratio between carbon dioxide and calcium carbonate is 1:1 and the molar mass of the reactant is 100 g/mol, the mass that yields such volume turns out:

$m_{CaCO_3}=1.79x10^{-3}molCO_2*\frac{1molCaCO_3}{1molCO_2} *\frac{100g CaCO_3}{1molCaCO_3}\\ \\m_{CaCO_3}=0.179gCaCO_3$

Regards.

3 0

4 years ago

A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is

Anuta_ua [19.1K]

The maximum safe operating temperature for this reaction is equal to 895°C.

Given the following data:

Width of cylinder = 22 cm.

Height, h = 26.4 cm.

Maximum safe pressure = 6.30mpa.

Mass = 0.537 kg.

Scientific data:

Ideal gas constant, R = 8.314 L-kPa/Kmol.

Molar mass of of dinitrogen monoxide ( $N_2F_2$ ) gas = 66 g/mol.

Radius, r = $\frac{width}{2} =\frac{22}{2} =11\;cm$

<h3>How to calculate the maximum safe operating temperature.</h3>

First of all, we would determine the volume of the stainless-steel cylinder by using this formula:

$V=\pi r^2 h\\\\V = 3.142 \times 11^2 \times 26.4\\\\$

Volume, V = 10,036.81 $cm^3$ .

In liters, we have:

Volume, V = 10.04 Liters.

Next, we would determine the number of moles of dinitrogen monoxide ( $N_2F_2$ ) gas:

$Number \;of \;moles = \frac {mass}{molar\;mass}\\\\Number \;of \;moles = \frac {537}{66}$

Number of moles = 8.136 moles.

Now, we can solve for the maximum safe operating temperature by applying the ideal gas equation:

$PV=nRT\\\\T=\frac{PV}{nR} \\\\T=\frac{6.30 \times 10^3 \times 10.04}{8.136 \times 8.314}\\\\T=\frac{60541.2}{67.6427}$

T = 895.02 ≈ 895°C.

Read more on temperature here: brainly.com/question/24769208

5 0

3 years ago