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artcher [175]
3 years ago
15

A sample of aluminum foil contains 7.90 x 10^23 atoms. What is the mass of the foil?

Chemistry
1 answer:
Zanzabum3 years ago
4 0

Answer:

35.3 g

Explanation:

Step 1: Given data

Number of atoms of aluminum: 7.90 × 10²³ atoms

Step 2: Calculate the number of moles corresponding to 7.90 × 10²³ atoms of aluminum

We will use Avogadro's number: there are 6.02 × 10²³ atoms of aluminum in 1 mole of atoms of aluminum.

7.90 × 10²³ atoms × (1 mol/6.02 × 10²³ atoms) = 1.31 mol

Step 3: Calculate the mass corresponding to 1.31 moles of aluminum

The molar mass of Al is 26.98 g/mol.

1.31 mol × 26.98 g/mol = 35.3 g

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ale4655 [162]
\hbox { You have to calculate the Molecular Mass for H2:}

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\hbox { So, in 2,0158 grames of H you will have 1 mole...}
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3 years ago
If the net force on a hot-air balloon is directed straight upward, which way does the acceleration point?
Marizza181 [45]

Answer:

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3 years ago
Carbon dioxide (CO2) is a gaseous compound. Calculate the percent composition of this compound. Answer using three significant f
Tamiku [17]

Carbon dioxide is a gaseous molecule made up of the elements, C and O. Each mole of carbon dioxide has one mole C and two mole oxygen atoms.

Molar mass of carbon dioxide (CO_{2})=(1 * 12.01\frac{g}{mol}) +(2* 16\frac{g}{mol})=44.01\frac{g}{mol}

Percentage by mass of carbon = \frac{(1*12.01\frac{g}{mol}) }{44.01\frac{g}{mol} } *100=27.3%

Percentage by mass of oxygen = \frac{(2*16\frac{g}{mol})}{44.01\frac{g}{mol} } *100=72.7%

Therefore C is 27.3 % and O is 72.7 % by mass in 1 mol CO_{2}

7 0
3 years ago
Read 2 more answers
1. For each of the molecules below, determine the electron geometry, molecule geometry, and bond
Alexxx [7]

Answer:

CCl4- tetrahedral bond angle 109°

PF3 - trigonal pyramidal bond angles less than 109°

OF2- Bent with bond angle much less than 109°

I3 - linear with bond angles = 180°

A molecule with two double bonds and no lone pairs - linear molecule with bond angle =180°

Explanation:

Valence shell electron-pair repulsion theory (VSEPR theory) helps us to predict the molecular shape, including bond angles around a central atom, of a molecule by examination of the number of bonds and lone electron pairs in its Lewis structure. The VSEPR model assumes that electron pairs in the valence shell of a central atom will adopt an arrangement which tends to minimize repulsions between these electron pairs by maximizing the distance between them. The electrons in the valence shell of a central atom are either bonding pairs of electrons, located primarily between bonded atoms, or lone pairs. The electrostatic repulsion of these electrons is reduced when the various regions of high electron density assume positions as far apart from each other as possible.

Lone pairs and multiple bonds are known to cause more repulsion than single bonds and bond pairs. Hence the presence of lone pairs or multiple bonds tend to distort the molecular geometry geometry away from that predicted on the basis of VSEPR theory. For instance CCl4 is tetrahedral with no lone pair and four regions of electron density around the central atom. This is the expected geometry. However OF2 also has four regions of electron density but has a bent structure. The molecule has four regions of electron density but two of them are lone pairs causing more repulsion. Hence the observed bond angle is less than 109°.

8 0
3 years ago
What type of elements are most likely to form more than one type of ion
ss7ja [257]
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7 0
3 years ago
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