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anyanavicka [17]

3 years ago

13

se tienen 10 litros de nitrogeno gaseoso bajo una presion de 560 mm Hg. Determina el volumen del nitrogeno a una presion de 760

mm Hg

1 answer:

Dominik [7]3 years ago

3 0

Answer:

working business city philadelphian

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A student measures the S2- concentration in a saturated aqueous solution of iron(II) sulfide to be 2.29×10-9 M. Based on her dat

katrin2010 [14]

Answer:

Ksp FeS = 5.2441 E-18

Explanation:

FeS ↔ Fe2+ + S2-

S S S

∴ Ksp = [Fe2+]*[S2-].....solubility product constant

∴ [S2-] = 2.29 E-9 M = S

⇒ Ksp = (S)(S) = S²

⇒ Ksp = (2.29 E-9)²

⇒ Ksp = 5.2441 E-18

8 0

3 years ago

The intermolecular forces present in CH 3NH 2 include which of the following? I. dipole-dipole II. ion-dipole III. dispersion IV

astra-53 [7]

Answer:

I. dipole-dipole

III. dispersion

IV. hydrogen bonding

Explanation:

Intermolecular forces are weak attraction force joining nonpolar and polar molecules together.

London Dispersion Forces are weak attraction force joining non-polar and polar molecules together. e.g O₂, H₂,N₂,Cl₂ and noble gases. The attractions here can be attributed to the fact that a non -polar molecule sometimes becomes polar because the constant motion of its electrons may lead to an uneven charge distribution at an instant.

Dispersion forces are the weakest of all electrical forces that act between atoms and molecules. The force is responsible for liquefaction or solidification of non-polar substances such as noble gas an halogen at low temperatures.

Dipole-Dipole Attractions are forces of attraction existing between polar molecules ( unsymmetrical molecules) i.e molecules that have permanent dipoles such as HCl, CH3NH2 . Such molecules line up such that the positive pole of one molecule attracts the negative pole of another.

Dipole - Dipole attractions are more stronger than the London dispersion forces but weaker than the attraction between full charges carried by ions in ionic crystal lattice.

Hydrogen Bonding is a dipole-dipole intermolecular attraction which occurs when hydrogen is covalently bonded to highly electronegative elements such as nitrogen, oxygen or fluorine. The highly electronegative elements have very strong affinity for electrons. Hence, they attracts the shared pair of electrons in the covalent bonds towards themselves, leaving a partial positive charge on the hydrogen atom and a partial negative charge on the electronegative atom ( nitrogen in the case of CH3NH2 ) . This attractive force is know as hydrogen bonding.

7 0

4 years ago

ANSWER ASAP GIVING BRAINLIEST FIVE STARS AND A HEART! Btw this is 6th grade science!

AlexFokin [52]

Answer:

Visible light.

Infrared waves.

X-rays.

Ultraviolet light.

Gamma rays.

Radio waves.

Microwaves.

Explanation:

6 0

3 years ago

A.<br> B.<br> C.<br> D.<br><br> Help me please?

Rina8888 [55]

Answer:

B: it allow quick conversation to others

6 0

3 years ago

Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s)+3Cl2(g)→2AlCl3(s) What is the max

jolli1 [7]

<u>Answer:</u> The mass of aluminium chloride that can be formed are 46.3 g

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ....(1)

<u>For Aluminium:</u>

Given mass of aluminium = 32 g

Molar mass of aluminium = 26.98 g/mol

Putting values in above equation, we get:

$\text{Moles of aluminium}=\frac{32g}{26.98g/mol}=1.186mol$

<u>For Chlorine:</u>

Given mass of chlorine = 37 g

Molar mass of chlorine = 71 g/mol

Putting values in above equation, we get:

$\text{Moles of chlorine gas}=\frac{37g}{71g/mol}=0.521mol$

For the given chemical equation:

$2Al(s)+3Cl_2(g)\rightarrow 2AlCl_3(s)$

By Stoichiometry of the reaction:

3 moles of chlorine gas is reacting with 2 moles of aluminium.

So, 0.521 moles of chlorine gas will react with = $\frac{2}{3}\times 0.521=0.347moles$ of aluminium.

As, given amount of aluminium is more than the required amount. Thus, it is considered as an excess reagent.

So, chlorine gas is considered as a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

3 moles of chlorine gas is producing 2 moles of aluminium chloride

So, 0.521 moles of chlorine gas will react with = $\frac{2}{3}\times 0.521=0.347moles$ of aluminium chloride.

Now, calculating the mass of aluminium chloride by using equation 1, we get:

Moles of aluminium chloride = 0.347 moles

Molar mass of aluminium chloride = 133.34 g/mol

Putting all the values in equation 1, we get:

$0.347mol=\frac{\text{Mass of aluminium chloride}}{133.34g/mol}\\\\\text{Mass of aluminium chloride}=46.3g$

Hence, the mass of aluminium chloride that can be formed are 46.3 g

7 0

4 years ago