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2 years ago

An ionic compound is typically made of

1 answer:

6 0

C. A metal and a non metal, the metal forms a positive ion (by transferring electrons to the non metal) and the non metal forms a negative ion (by gaining the electrons from the non metal). The oppositely charged ions strongly attract each other.

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n-Butane (C4H10) is burned with stoichiometric amount of oxygen. Determine the mole fraction of carbon dioxide and water in the

Fudgin [204]

Answer:

See details below

Explanation:

The balanced reaction equation is given below:

$2C_{4} H_{10}$ + $13O_{2}$ → $8CO_{2}$ + $10H_{2} O$

Mole fraction of CO2 to H20

= 8/10 = $\frac{4}{5}$

Mole ratio of C4H10 to CO2 is 2:8 = 1:4

1 mole of n-butane - 38.12 g

4 moles - ?

= 152.48g fuel consumed.

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3 years ago

Q. Which of the following scenarios describes a process with a negative system entropy change?

Westkost [7]

A. Building a skyscraper.

8 0

2 years ago

Read 2 more answers

balance the following reaction. a coefficient of "1" is understood. choose option "blank" for the correct answer if the coeffici

suter [353]

Balanced chemical reaction: 2KCl + Pb(NO₃)₂ → PbCl₂ + 2KNO₃.

According to principle of mass conservation, number of atoms must be equal on both side of balanced chemical reaction.

KCl is potassium chloride.

Pb(NO₃)₂ is lead(II) nitrate.

KNO₃ is potassium nitrate.

PbCl₂ is lead(II) chloride.

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2 years ago

The iodine "clock reaction" involves the following sequence of reactions occurring in a reaction mixture in a single beaker. 1.

Mars2501 [29]

C: 0.012 mol.

<h3>Explanation</h3>

Start with 0.0020 moles of iodate ions ${\text{IO}_{3}}^{-}$ .

How many moles of iodine $\text{I}_2$ will be produced?

${\text{IO}_{3}}^{-}$ converts to $\text{I}_2$ in the first reaction. The coefficient in front of $\text{I}_2$ is three times the coefficient in front of ${\text{IO}_{3}}^{-}$ . In other words, each mole of ${\text{IO}_{3}}^{-}$ will produce three moles of $\text{I}_2$ . 0.0020 moles of ${\text{IO}_{3}}^{-}$ will convert to 0.0060 moles of $\text{I}_2$ .

How many moles of thiosulfate ions ${\text{S}_2\text{O}_3}^{2-}$ are required?

$\text{I}_2$ reacts with ${\text{S}_2\text{O}_3}^{2-}$ in the second reaction. The coefficient in front of $\text{I}_2$ is twice the coefficient in front of ${\text{S}_2\text{O}_3}^{2-}$ . How many moles of ${\text{S}_2\text{O}_3}^{2-}$ does each mole of $\text{I}_2$ consume? Two. 0.0060 moles of $\text{I}_2$ will be produced. As a result, $2 \times 0.0060 = 0.0120$ moles of ${\text{S}_2\text{O}_3}^{2-}$ will be needed.

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2 years ago

Calculate the normality of a solution containing 147 g of h2s04 in 2L of solution

babunello [35]

I am not sure plz show me the question

5 0

3 years ago