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3 years ago

Type the chemical name of the compound that contains 1 copper atom, 1 oxygen

Chemistry

1 answer:

Bas_tet [7]3 years ago

4 0

Answer:

Copper (I) hydroxide

Explanation:

Copper (I) hydroxide is a chemical compound with the chemical formula of CuOH. One copper atom (Cu), one oxygen atom (O), and one hydrogen atom (H.)

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2.173 moles of ethanol is presented in a 100.0g sample of ethanol .

Explanation:

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3 years ago

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3 years ago

Metallic bonds form between what kinds of atoms?

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2 years ago

Read 2 more answers

A pure copper penny contains approximately 2.9×1022 copper atoms. Use the following definitions to determine how many ______ of

hammer [34]

Complete question is;

A pure copper penny contains approximately 2.9 × 10^(22) copper atoms.

1 doz = 12

1 gross = 144

1 ream = 500

1 mol = 6.022 × 10^(23)

Use these definitions to determine the following:

A) How many dozens of copper atoms are in a penny.

B) How many gross of copper atoms are in a penny

C) How many reams of copper atoms are in a penny.

D) how many moles of copper atoms are in a penny?

All answers can be rounded to two significant figures

Answer:

A) 2.4 × 10^(21) dozens

B) 2.01 × 10^(20) gross

C) 5.8 × 10^(19) reams

D) 0.048 mol

Explanation:

A) A dozen contains 12.

Therefore, 2.9 × 10^(22) copper atoms will contain;

(2.9 × 10^(22))/12 dozens = 2.42 × 10^(21).

In 2 significant figures, we have;

2.4 × 10^(21) dozens

B) 1 gross = 144

Therefore, 2.9 × 10^(22) copper atoms will contain;

(2.9 × 10^(22))/144 gross ≈ 2.01 × 10^(20) gross

C) 1 ream = 500

Therefore, 2.9 × 10^(22) copper atoms will contain;

(2.9 × 10^(22))/500 reams = 5.8 × 10^(19) reams

D) 1 mol = 6.022 × 10^(23)

Therefore, 2.9 × 10^(22) copper atoms will contain;

(2.9 × 10^(22))/(6.022 × 10^(23)) = 0.048 mol

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3 years ago

Calculate the energy required to produce 7.00 mol Cl2O7 on the basis of the following balanced equation. 2Cl2(g) + 7O2(g) + 130

KatRina [158]

Explanation:

As the given chemical reaction equation is as follows.

$2Cl_{2}(g) + 7O_{2}(g) + 130 kcal \rightarrow 2Cl_{2}O_{7}(g)$

Also, it is given that for 2 moles the energy required is 130 kcal. This means that energy required for 1 mole is calculated as follows.

1 mole = $\frac{130 kcal}{2}$

= 65 kcal

Hence, energy required for 7 moles will be calculated as follows.

Energy required = $7 \times 65 kcal$

= 455 kcal

Thus, we can conclude that energy required to produce 7.00 mol $Cl_{2}O_{7}$ on the basis of given reaction is 455 kcal.

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3 years ago