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borishaifa [10]

3 years ago

15

what does NaBr + Ca(OH)2 -> CaBr2 + NaOH make, what rection for an example rust. is it aa chemical reaction? please reply asa

p ty sm

2 answers:

yuradex [85]3 years ago

4 0

Formula for rust is FE203.XH20.

Semenov [28]3 years ago

3 0

FORMULA FOR RUST IS FE2O3.XH20

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Reaccionan 54gr de Nitrato de plata al 39 % de pureza, con 72gr de ácido clorhídrico al 83% de pureza, en un proceso donde se ob

netineya [11]

Answer:Reaccionan 54gr de Nitrato de plata al 39 % de pureza, con 72gr de ácido clorhídrico al 83% de pureza, en un proceso donde se obtienen 93 gr de cloruro de - 154… ... 93 gr de cloruro de plata. El otro producto es el ácido nítrico: Calcular el porcentaje de rendimiento de la reacción y balancearlo.

6 0

2 years ago

A flashlight battery is hooked to a toy motor, and then the battery and the connections are sprayed with a water-proof coating.

denis-greek [22]

Explanation:

Formula to calculate work done by motor is as follows.

Work done by motor = $mass \times g \times height$

where, g = gravitational constant = 10 $m/s^{2}$

Therefore, work done by motor is as follows.

Work done by motor = $1.00 kg \times 10 m/s^{2} \times 10.0 m$

= 100.0 J

Now, heat lost by water will be calculated as follows.

q = $mC \times \Delta T$

= $g \times 4.184 J/g^{o}C \times 0.024^{o}C$

= 10.0 J

Hence, heat gained by motor = heat lost by water

As, heat gained by motor = 10.0 J

So, change in energy = heat gained - work done

Therefore, change in energy will be calculated as follows.

Change in energy = heat gained - work done

= (10.0 J) - (100.0 J)

= -90.0 J

Thus, we can conclude that change in the energy of the battery contents is -90.0 J.

4 0

2 years ago

to show the electron configuration for an atom, when would it be better to use an orbital notation than to use a written configu

sineoko [7]

The aim is to use less space while demonstrating the distribution of electrons in shells

If you want to depict how an atom's electrons are scattered across its subshells, an orbital notation is more suited.

This is due to the fact that some atoms have unique electronic configurations that are not readily apparent from textual configurations.

<h3>How does electron configuration work?</h3>

The placement of electrons in orbitals surrounding an atomic nucleus is known as electronic configuration, also known as electronic structure or electron configuration.

<h3>What sort of electron arrangement would that look like?</h3>

For instance: You can see that oxygen contains 8 electrons on the periodic table.
These 8 electrons would fill in the following order: 1s, 2s, and finally 2p, according to the aforementioned fill order. O 1s22s22p4 would be oxygen's electron configuration.

learn more about electronic configuration here

brainly.com/question/26084288

#SPJ4

7 0

1 year ago

_____ is the measure of the degree of charge separation within a polar molecule.

yawa3891 [41]

Your answer is .....

The dipole Moment

Good luck! :)

7 0

2 years ago

Read 2 more answers

Calculate the mass of excess reagent remaining at the end of the reaction in which 90.0 g of SO2 are mixed with 100.0 g of O2

Radda [10]

We have to first write a balanced equation.
so2 + o2 -> so3

this is not balanced though. we have 3 oxygen on right and 4 on left
2so2 + o2 -> 2so3

now it is same on both sides. we have to figure out which is limiting reagent with the given amounts of reagents. we do this by comparing the ratio between them in terms of moles. we see that so2 has a coefficient of 2 and o2 has none which implies 1 and so3 has 2. this means that for every 2 moles of so2 reacting with 1 mole of o2, we get 2 moles of so3.

lets convert the given values to moles. to do this we know that molecular weight is measured in grams per mole. we are given grams and need to cancel out the grams to get moles. so the molecular weight:
so2 =32.1 + 2 * 16 = 64.1 g/mol
o2 = 2 * 16 = 32 g/mol
so3 = 32.1 + 3 * 16 = 80.1 g/mol

now to convert 90 g of 2so2 under ideal conditions.
90g / 64.1g/mol = 1.404 moles

convert this amount of moles of so2 to moles of o2. we have 2 moles of so2 to 1 of o2
1.404moles so2 / 2 moles so2 * 1 mole o2= 0.702 moles o2

so we see under ideal conditions that 90g of so2 would react with .702g of o2. lets see how many we actually have with 100g of o2
100g / 32g/mol =3.16 mol.

so we have a lot more o2 than needed. we are looking for how much is left in grams. we have to figure out how much was used. to do this convert our ideal moles of o2 into grams.
.702 moles o2 * 32g/mol = 22.5g o2

so what we startrd with (100g) minus what we needed (22.5g) is what we have left
100 - 22.5 = 77.5g o2

6 0

2 years ago