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yanalaym [24]
3 years ago
15

Which of the following elements is a nonmetal? a. selenium (Se) b. yttrium (Y) c. barium (Ba) d. calcium (Ca) e. All of these ar

e metals.
Chemistry
2 answers:
Fynjy0 [20]3 years ago
8 0

Answer:

a. Selenium

Explanation:

Selenium is a non metal but though rarely, it is considered to be a metalloid.

(Metalloids are elements intermediate between metals and nonmetals and are known to have partly metallic and partly non metallic properties.)

Selenium is in group 16 of the periodic table below sulphur and has average properties of the group elements above and below it in the periodic table..  

san4es73 [151]3 years ago
3 0

<u>Answer:</u>

The correct answer option is a. Selenium (Se).

<u>Explanation:</u>

From the given answer options, Selenium (Se) is the only element which is a non metal.

It has the atomic number 34 with atomic weight 78.96. It is a member of the sulfur group of the non metallic elements and falls in period 4 of the Periodic table.

Selenium has non metallic properties which are intermediate between the elements that lie above and below it in the Periodic table.

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A reaction occurs when one compound reacts and is broken down into different elements or simpler compounds.
Inessa [10]

Answer:

Decomposition Reaction

Explanation:

If you are referring to what type of reaction that occurred then the answer would be decomposition reaction.

This is a chemical reaction where one reactant is broken down into two or more products.

REACTANT → PRODUCT

       AB       →      A + B

The products can be two or more elements or two or more compounds, depending on what was decomposed.

3 0
3 years ago
Read 2 more answers
onsider the following reaction: CaCN2 + 3 H2O → CaCO3 + 2 NH3 105.0 g CaCN2 and 78.0 g H2O are reacted. Assuming 100% efficiency
mestny [16]

Answer : The excess reactant is, H_2O

The leftover amount of excess reagent is, 7.2 grams.

Solution : Given,

Mass of CaCN_2 = 105.0 g

Mass of H_2O = 78.0 g

Molar mass of CaCN_2 = 80.11 g/mole

Molar mass of H_2O = 18 g/mole

Molar mass of CaCO_3 = 100.09 g/mole

First we have to calculate the moles of CaCN_2 and H_2O.

\text{ Moles of }CaCN_2=\frac{\text{ Mass of }CaCN_2}{\text{ Molar mass of }CaCN_2}=\frac{105.0g}{80.11g/mole}=1.31moles

\text{ Moles of }H_2O=\frac{\text{ Mass of }H_2O}{\text{ Molar mass of }H_2O}=\frac{78.0g}{18g/mole}=4.33moles

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

CaCN_2+3H_2O\rightarrow CaCO_3+2NH_3

From the balanced reaction we conclude that

As, 1 mole of CaCN_2 react with 3 mole of H_2O

So, 1.31 moles of CaCN_2 react with 1.31\times 3=3.93 moles of H_2O

From this we conclude that, H_2O is an excess reagent because the given moles are greater than the required moles and CaCN_2 is a limiting reagent and it limits the formation of product.

Left moles of excess reactant = 4.33 - 3.93 = 0.4 moles

Now we have to calculate the mass of excess reactant.

\text{ Mass of excess reactant}=\text{ Moles of excess reactant}\times \text{ Molar mass of excess reactant}(H_2O)

\text{ Mass of excess reactant}=(0.4moles)\times (18g/mole)=7.2g

Thus, the leftover amount of excess reagent is, 7.2 grams.

8 0
3 years ago
I'll mark brainliest!! :)
Viefleur [7K]
I believe the answer is C, AgBr. I hope this helps
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1362205.2 in scientific notation
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1.3622052x10^6 you move the . 6 places to the left making it a positive 10^6
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H-C C-H name of formula
Vanyuwa [196]

Answer:

Ethyne

Explanation:

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