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3 years ago

Which of the following is an element?

Chemistry

2 answers:

antiseptic1488 [7]3 years ago

7 0

Answer:

A.) Zinc (Zn) is a metal

Explanation:

Hope this helps!

wlad13 [49]3 years ago

4 0

Answer:

A. zinc metal

Explanation:

Zinc is a chemical element with the symbol Zn and atomic number 30. Zinc is a slightly brittle metal at room temperature and has a blue-silvery appearance when oxidation is removed. It is the first element in group 12 of the periodic table.

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What happens to valence electrons in ionic bonding? this is a question i know but gives me answer choices im not sure about

il63 [147K]

I think the answer is B, the metal loses valence electrons to the nonmetal.

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3 years ago

How many electrons can occupy the s orbitals at each energy level?

PtichkaEL [24]

The atomic orbital is describes using the principle quantum number followed by a letter (s, p, d or f) that describe the sublevel.

For sublevel, it has the shape of a spherical electron cloud surrounding the nucleus and it can hold up to two electrons.

Therefore, the answer to your question is 2 electrons.

6 0

4 years ago

Calculate the number of molecules 2.62x10^-6g of water, H2O

bagirrra123 [75]

87.33 X 10^15 molecules

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4 years ago

Sixty-three grams of copper reacted with 32 grams of sulfur. this chemical reaction produced the compound copper sulfide. what w

Nuetrik [128]

The mass of, $Cu_2S$ , compound formed is 77.9g

62 grams of copper reacted with 32grams of sulfur to form copper sulfide.

$Cu + S_2 \rightarrow CuS_2$

stoichiometry of Cu to S is 2:1

We need to find the limiting reactant

Molar mass of copper = 63.5 g/mol

Molar mass of Sulfur = 32 g/mol

Number of moles of Copper = $\dfrac{mass} {molar mass } = 0.99mole$

Number of moles of Sulfur = $\dfrac{mass} {molar mass} = \dfrac{32g} {32g/mol} = 1 mole$

Since copper have lesser number of moles, therefore the limiting reagent is copper so the amount of product formed depends on amount of Cu present

stoichiometry of Copper to $Cu_2S$ is 2:1

0.99 mol of Copper forms = $\dfrac{0.99} {2}$ = 0.49 mol of $Cu_2S$

Mass of $Cu_2S$ produced = Number of moles $\times$ Molar mass

Mass of $Cu_2S$ produced = 0.49 mol $\times$ 159 g/mol = 77.9g

Learn more about limiting reagent here-

brainly.com/question/9913056

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6 0

2 years ago

At 500°C the equilibrium constant, Kp, is 4.00 × 10–4 for the equilibrium: 2HCN(g) H2(g) + C2N2(g) What is Kp for the following

Andrews [41]

Answer: The value of $K_p$ for the equation is $2.5\times 10^3$

Explanation:

The given chemical reaction is:

$2HCN(g)\rightleftharpoons H_2(g)+C_2N_2(g);K_1$

The chemical equation for which the equilibrium constant is to be calculated follows:

$H_2(g)+C_2N_2(g)\rightleftharpoons 2HCN(g);K_p$

As, the equation is the result of the reverse of given reaction. So, the equilibrium constant for the equation will be the inverse of equilibrium constant for the given reaction.

The value of equilibrium constant for the equation is:

$K_p=\frac{1}{K_1}$

We are given:

$K_1=4.00\times 10^{-4}$

Putting values in above equation, we get:

$K_p=\frac{1}{4.00\times 10^{-4}}=2.5\times 10^3$

Hence, the value of $K_p$ for the equation is $2.5\times 10^3$

3 0

4 years ago