All categories

3 years ago

Which nonmetal has the greatest potential to be oxidized

Chemistry

1 answer:

Tasya [4]3 years ago

7 0

Answer:

Hydrogen

Explanation:

A reducing agent is a substance which gives up its electrons to become oxidized. Generally, metals are oxidized (reducing agents) while non-metals are reduced (oxidizing agents).

However, hydrogen which is a non-metal is usually oxidized in the presence of stronger oxidizing non-metals such as fluorine and oxygen.

Hydrogen thus, acts as a reducing agent by giving up its electrons to become oxidized. Even though among all non-metals, Hydrogen has the greatest potential to be oxidized, it is a poor reducing agent compared to reactive metals.

You might be interested in

What phenomenon does the Coriolis effect arise from?

Andre45 [30]

Answer:

because our planet is spinning

which means the objects near the equator are moving at much faster velocities than objects at higher latitudes

I hope this helps✌

7 0

2 years ago

A gymnast performing a backflip into a cartwheel on a balance beam is am example of ________ force

Angelina_Jolie [31]

I’m gonna guess equal force sorry if I get it wrong <3

8 0

2 years ago

Indenting the type of weathering seen in each picture

svetoff [14.1K]

Answer:

What picture ?

Explanation:

3 0

3 years ago

1. A chemist prepares hydrogen fluoride by means of the following reaction:

Natasha_Volkova [10]

Answer:

a) Theoretical Yield of HF = 5.64 grams

b) Percentage Yield = 39%

Explanation:

Reaction Given:

CaF2 + H2SO4 -> CaSO4 + 2HF

CaF2 = 11g

H2SO4 = Used in excess

HF = 2.2 g production = Actual Yield

So, Let's write down the molar masses:

Molar Mass of CaF2 = 78 g /mol

Molar Mass of HF = 20 g/mol

From the reaction, we can see the 1 mole of CaF2 gives the 2 moles of HF

i.e

a) Theoretical Yield of HF:

1 mole CaF2 = 2 moles HF

78 g CaF2 = 2 x 20 g of HF

78 g CaF2 = 40 g of HF

1 g CaF2 = 40g/78g of HF

And in the question it is given that chemist used 11 g of CaF2 so,

1 x 11 g of CaF2 = 11 x 40/78 g of HF

11 g of CaF2 = 440/78 g of HF

11 g of CaF2 = 5.64 g of HF

And this is the theoretical yield

Theoretical Yield of HF = 5.64 grams

b) Now, calculate the Percentage Yield of HF

Percentage Yield = Actual Yield /Theoretical Yield x 100

Percentage Yield = 2.2 g /5.64 g x 100

Percentage Yield = 39%

8 0

2 years ago

PLEASE HELP!!! The image represents the reaction between a certain number of molecules of N2 and H2.

77julia77 [94]

Answer:

The leftover reactant is the nitrogen gas, N₂.

Explanation:

As per your description:

1. Square on the left: N₂(g)

3 units of two joint circles: this represents 3 molecules of nitrogen gas, N₂(g).

2. Square on the right: H₂(g)

3 units of two joint circles: this represents 3 molecules of hydrogen gas, H₂(g).

3. Reaction

If the maximum possible amount of NH₃ is formed during the reaction, you assume that the reaction goes to completion.

The chemical equation that represents the reaction is:

N₂(g) + H₂(g) → NH₃(g)

Which must be balanced:

N₂(g) + 3H₂(g) → 2NH₃(g)

That means that 1 molecule (or 1 mol) of N₂(g) reacts with 3 molecules (or 3 moles ) of H₂(g) to produce 2 molecules (or 2 moles) of NH₃(g).

Since, the squares show that there are 3 molecules of each reactant, the 3 molecules of hydrogen gas will be able to react with 1 molecule of nitrogen gas. When that happens, all the hydrogen gas is consumend and yet two molecules of nitrogen gas will remain unreacted. Hence, the nitrogen gas is the leftover reactant.

4 0

3 years ago

Read 2 more answers