Someone help me please?

Answer:

10 moles of S₈

320 moles O₂

Explanation:

The balanced equation is:

Now we can convert moles of SO₈ (the product) into moles of each reactant, using the stoichiometric coefficients of the balanced reaction:

In order for 80 moles of SO₈ to be produced, 10 moles of S₈ need to react with 320 moles of O₂.

Answer:

75m

Explanation:

Answer:

true

Explanation:

Answer:

false

Explanation:

Sedimentary rocks form by breaking down other kinds of rocks into small particles and washing or blowing them away; metamorphic rocks form from other rocks and igneous rocks form by melting other rocks. ... Igneous Rocks: form by crystallizing melted material (magma).

Answer:

3.     c

4.     d

5.     c

Explanation:

Answer:gear

Explanation:just did it right now

Answer: Gear

Explanation: just did it on Edge 2021

Answer:

red dwarf

Explanation:

Answer:

D

Explanation:

Answer:

19.45g of Cu are expect to be produced

Explanation:

Based on the reaction:

2Ni + 3CuCl2 → 3Cu + 2NiCl3

2 moles of Ni react with 3 moles of CuCl2 to produce 3 moles of Cu

To solve this question we must find the moles of each reactant in order to find the limiting reactant. With the limiting reactant we can find the moles of Cu produced and the mass as follows:

Moles Ni -Molar mass: 58.6934g/mol-

12.00g * (1mol / 58.6934g) = 0.204 moles Ni

Moles CuCl2 -Molar mass: 134.45g/mol-

42.00g * (1mol / 134.45g) = 0.312 moles CuCl2

For a complete reaction of 0.204 moles of Ni are required:

0.204 moles Ni * (3 moles CuCl2 / 2 moles Ni) = 0.306 moles of CuCl2

As there are 0.312 moles, CuCl2 is the excess reactant and Ni is limiting reactant.

Moles Cu:

0.204 moles Ni * (3moles Cu / 2 moles Ni) = 0.306 moles of Cu are produced

Mass Cu:

0.306 moles of Cu * (63.546g / mol) =

Answer:

C. 33.6L

Explanation:

Based on the reaction, 2 moles of HCl reacts producing 1 mole of hydrogen.

To solve this question we must find the moles of hydrogen produced using the reaction. Then, with combined gas law (PV = nRT) we can find the volume produced:

Moles H2:

3.00 moles HCl * (1mol H2 / 2mol HCl) = 1.50 moles H2 are produced

Volume:

PV = nRT

V = nRT / P

Where P is pressure = 1atm at STP

V is volume = Our incognite

n are moles of the gas = 1.50 moles

R is gas constant = 0.082atmL/molK

T is absolute temperature = 273.15K

V = nRT / P

V = 1.50mol*0.082atmL/molK*273.15K / 1atm

V = 33.6L

Answer:

Solids, liquids, gases - all matter - are made up of atoms (or other things, like molecules, that are made from atoms)! ELEMENTS are the kinds of atoms that we can have. Carbon is an element, hydrogen is an element, and so is oxygen. ... Atoms can join together - they form bonds together - to make MOLECULES.

Answer:

a. Sn or Si ⇒ Sn

b. Br or Ga ⇒ Ga

c. Sn or Bi ⇒ similar in size

d. Se or Sn ⇒ Sn

Explanation:

The larger atom has a larger atomic radius. We have to consider how varies the atomic radius for chemical elements in the Periodic Table. In a group (column), the atomic radius increases from top to bottom while in a period (file), it increases from right to left.

a. Sn or Si ⇒ Sn

They are in the same group. Sn is on the top, so it has a larger atomic radius.

b. Br or Ga ⇒ Ga

They are in the same period. Ga is located at the left so it has a larger atomic radius.

c. Sn or Bi ⇒ similar

They are not in the same group neither the same period. Bi is located more at the bottom, so it would be larger than Sn, but Bi is also at the right side, so it would be smaller than Bi. Thus, they have comparable sizes.

d. Se or Sn⇒ Sn

They are not in the same group neither the same period. Se is located at the top and right side compared to Sn, so Sn is the larger atom.

Answer:

  2 Atm; 2.016 g

Explanation:

Changing the volume without changing the temperature or mass only changes the pressure. Volume and pressure are inversely proportional so halving the volume will double the pressure.

P = 1 Atm, T = 0 °C are "standard" temperature and pressure (STP). The volume of 1 mole of gas is 22.4 L under these conditions. That means the amount of hydrogen gas in the cylinder is 1 mole, so has a mass of 2.016 g.

After the volume reduction, the pressure is 2 Atm, and the mass remains 2.016 g.

Answer:

Explanation:

hope it helps

Answer:

(with reference to a solid) become or cause to become incorporated into a liquid so as to form a solution.

Answer:

The equilibrium position shifts to the right.

This is due to excess carbon dioxide which supresses the reaction.

C. Venus is the answer..

Answer:

Food storage. The food reserves can be drawn upon to ensure good development of a flower stalk and seeds.

Explanation:

Hope this helps!

Answer:

Geothermal energy is an uptrending alternative source of production that relies on the earth's crust and elements of radioactivity.

Answer:

two smaller, more stable nuclei

Explanation:

A. two smaller, more stable nuclei

Nuclear fission is the process in which a heavy nucleus is split into two large fragments of comparable mass to form more stable and smaller nuclei. This results in the release of great amounts of energy. Large nuclei are usually less stable, since it takes more energy to hold its structure together, the larger they are.

Here's a photo of Edge just incase.

Explanation:

No of moles = mass/ molar mass

MgCl2 = 24+35.5*2

= 24+70

= 94 gmol—1

No of moles = 1.25/94

= 0.013 moles

One mole of magnesium chloride weighs 95.21 grams. Therefore, the number of moles in  1.25 grams of the compound is 0.0131 moles.

Magnesium chloride is an ionic compound formed by the electron transfer from magnesium metal to the chlorine atoms.

To determine the number of moles of MgCl₂ in 1.25 grams, we need to use the formula:

moles = mass / molar mass

The molar mass of MgCl₂ can be calculated by adding up the atomic masses of its constituent atoms, which are:

Mg: 24.31 g/mol

Cl: 35.45 g/mol (x2, since there are two Cl atoms in MgCl2)

So, the molar mass of MgCl₂ is:

MgCl₂: 24.31 g/mol + 35.45 g/mol x 2 = 95.21 g/mol

Now we can use the formula to calculate the number of moles:

moles = mass / molar mass = 1.25 g / 95.21 g/mol

moles = 0.0131 mol (rounded to four significant figures)

Therefore, there are approximately 0.0131 moles of MgCl₂ in 1.25 grams.

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Answer:

11.9 g of nitrogen monoxide

Explanation:

We'll begin by calculating the number of mole in 6.75 g of NH₃. This can be obtained as follow:

Mass of NH₃ = 6.75 g

Molar mass of NH₃ = 14 + (3×1)

= 14 + 3

= 17 g/mol

Mole of NH₃ =?

Mole = mass /molar mass

Mole of NH₃ = 6.75 / 17

Mole of NH₃ = 0.397 mole

Next, we shall determine the number of mole of NO produced by the reaction of 0.397 mole of NH₃. This can be obtained as follow:

4NH₃ + 5O₂ —> 4NO + 6H₂O

From the balanced equation above,

4 moles of NH₃ reacted to produce 4 moles of NO.

Therefore, 0.397 mole of NH₃ will also react to produce 0.397 mole of NO.

Finally, we shall determine the mass of 0.397 mole of NO. This can be obtained as follow:

Mole of NO = 0.397 mole

Molar mass of NO = 14 + 16 = 30 g/mol

Mass of NO =?

Mass = mole × molar mass

Mass of NO = 0.397 × 30

Mass of NO = 11.9 g

Thus, the mass of NO produced is 11.9 g

Answer:

The concentration will be "[tex]1.88\times 10^5 \ ppm[/tex]".

Explanation:

The given values are:

Mass of solute (KNO₃),

= 15.0 grams

Mass of solvent (H₂O),

= 65.0 grams

The concentration will be:

=  [tex]\frac{Mass \ of \ solute}{Mass \ of \ solution}\times 10^6[/tex]

On substituting the values, we get

=  [tex]\frac{15.0}{65.0+15.0}\times 10^6[/tex]

=  [tex]\frac{15.0}{80}\times 10^6[/tex]

=  [tex]0.1875\times 10^6[/tex]

=  [tex]187500 \ ppm[/tex]

or,

=  [tex]1.88\times 10^5 \ ppm[/tex]

Answer:

3.04 mol NH3* (17.03 g NH3/ 1 mol NH3)= 51.8 g NH3~

The mass in grams of 3.04 mol of ammonia vapor is 51.68g

The mole is an amount unit similar to familiar units like pair, dozen, gross, etc. It provides a specific measure of the number of atoms or molecules in a bulk sample of matter.

A mole is defined as the amount of substance containing the same number of atoms, molecules, ions, etc. as the number of atoms in a sample of pure 12C weighing exactly 12 g.

Given,

Moles of ammonia = 3.04 moles

Molar mass of ammonia = 14 + 3 = 17

Moles = mass / molar mass

Mass = moles × molar mass

= 3.04 × 17

= 51.68 g

Therefore, mass in grams of 3.04 mol of ammonia vapor is 51.68g

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Answer:

74.99g

Explanation:

Mass of a substance can be calculated by using the formula;

mole = mass ÷ molar mass

mass = molar mass × mole

According to this question, 37.2 moles of hydrogen gas is given.

Molar mass of hydrogen gas (H2) = 1.008(2) = 2.016g/mol

mass = 2.016 × 37.2

Mass of H2 = 74.995

Mass = 74.99g

Answer:

2.7*10^-13

coefficient= 2.7

exponent= -13

Explanation:

Answer: 2.7 x 10^-13

Explanation:

Answer:

4.90 x 10 24 atoms

Explanation:

the 24 is the exponent for the 10

Answer: C

Explanation: The evaporation rate depends on the exposed surface of liquid as long as both glasses stay at the same temperature. Since both glasses have the same surface area, they should both evaporate at the same rate.

We want to solve Q = mcΔT for the liquid water; its change in temperature will tell us the amount of thermal energy that flowed out of the reaction. The specific heat, c, of water is 4.184 J/g °C.

Q = (72.0 g)(4.184 J/g °C)(100 °C - 25 °C) = 22593.6 J

Q ≈ 2.26 × 10⁴ J or 22.6 kJ (three significant figures).

Answer:

The atomic weight Ar, of M is 64

Explanation:

The formula of the given compound is M(OH)₂

Mr, is the molecular weight of a compound and for the given compound, Mr is equal to 98.

Ar, is the atomic weight of the elements in the compound

The molecular weight, Mrof a compound is the mass of one mole mole of that compound. It can be obtained by summing the atomic masses of all elements in that compound. For elements that has more than one atom in the compound, the atomic weight of that element is multiplied by the number of atoms of the element present in the compound and then the sum of the weight of each element gives the molecular weight of the compound.

Onnthe compound above,the atomic weight of the unknown element M, is to be obtained.

Ar of the other elements inn he compound is given : Ar of O = 16, Ar of H = 1.

Molecular weight of the compound, Mr = 98

Calculating for the Ar of M:

(M × 1) + (16 × 2) + (1 × 2) = 98

M +32 + 2 = 98

M + 34 = 98

M = 98 -34

M = 64

Therefore, the atomic weight Ar, of M is 64

Answer:

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