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3 years ago

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24. Which of the following pairs of solutions produce a precipitate when combined? A) Fe(NO); and KCI B) NH4Cl and AgNO3 C) KOH

and NH C1 D) Na2SO, and KC1 /

1 answer:

11Alexandr11 [23.1K]3 years ago

4 0

Answer:

69 my Nigerian brotherzzzzzzzz

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Science Experiment : What can you fit in your mouth?

IceJOKER [234]

Answer:

u got a me off guard and thought sum else, lol but um a marble?

Explanation:

5 0

3 years ago

For the given reactions, classify the reactants as the reducing agent, oxidizing agent, or neither.

3241004551 [841]

Answer: For $F_{2} + H_{2} \rightarrow 2HF$ , $F_{2}$ is the oxidizing agent and $H_{2}$ is the reducing agent.

For $2Mg + O_{2} \rightarrow 2MgO$ , Mg is the reducing agent and $O_{2}$ is the oxidizing agent.

Explanation:

An oxidizing agent is defined as the substance which tends to oxidize other substances by itself gaining electrons. As a result, there will occur a decrease in its oxidation state.

On the other hand, a substance which tends to reduce other substances by itself losing electrons is known as an reducing agent. There will occur an increase in oxidation state of a reducing agent.

For example, $F_{2} + H_{2} \rightarrow 2HF$

Oxidation: $H_{2} \rightarrow 2H^{+} + 2e^{-}$

Reduction: $F + 1e^{-} \rightarrow F^{-}$

Hence, here $F_{2}$ is the oxidizing agent and $H_{2}$ is the reducing agent.

Also,

$2Mg + O_{2} \rightarrow 2MgO$

Oxidation: $Mg \rightarrow Mg^{2+} + 2e^{-}$

Reduction: $O_{2} + 2e^{-} \rightarrow O$

Hence, here Mg is the reducing agent and $O_{2}$ is the oxidizing agent.

6 0

4 years ago

You are running a rather large scale reaction where you prepare the grignard reagent phenylmagnesium bromide by reacting 210.14

almond37 [142]

Answer:

We would expect to form 7.35 moles of grignard reagent.

Explanation:

<u>Step 1: </u>Data given

Mass of magnesium = 210.14 grams

Volume bromobenzene = 772 mL

Density of bromobenzene = 1.495 g/mL

Molar mass of Mg = 24.3 g/mol

Molar mass of bromobenzene = 157.01 g/mol

<u>Step 2</u>: The balanced equation

C6H5Br + Mg ⇒ C6H5MgBr

<u>Step 3:</u> Calculate mass of bromobenzene

Mass bromobenzene = density bromobenzene * volume

Mass bromobenzene = 1.495 g/mL * 772 mL

Mass bromobenzene = 1154.14 grams

<u>Step 4</u>: Calculate number of moles bromobenzene

Moles bromobenzene = mass bromobenzene / molar mass bromobenzene

Moles bromobenzene = 1154.14g / 157.01 g/mol

Moles bromobenzene = 7.35 moles

<u>Step 5:</u> Calculate moles of Mg

Moles Mg = 210.14 grams /24.3 g/mol

Moles Mg = 8.65 moles

<u>Step 6:</u> The limiting reactant

The mole ratio is 1:1 So the bromobenzene has the smallest amount of moles, so it's the limiting reactant. It will be completely consumed ( 7.35 moles). Magnesium is in excess, There will react 7.35 moles. There will remain 8.65 - 7.35 = 1.30 moles

<u>Step 7:</u> Calculate moles of phenylmagnesium bromide

For 1 mole of bromobenzene, we need 1 mole of Mg to produce 1 mole of phenylmagnesium bromide

For 7.35 moles bromobenzene, we have 7.35 moles phenylmagnesium bromide

We would expect to form 7.35 moles of grignard reagent.

5 0

3 years ago

Convert 3.01€22 molecules of O²(a) mole of O²) ,volume at S.T.P,no of Oxygen atom. (d) mass

Marat540 [252]

Answer:

a )0.05 moles of O₂

b) 1.1207 dm³

c) 0.3× 10²³ atoms of oxygen

d) 1.6 g

Explanation:

Given data:

Number of molecules of O₂ = 3.01 × 10²² molecules

Number of moles of O₂ = ?

Volume of oxygen at ATP = ?

Number of oxygen atoms = ?

Mass of oxygen = ?

Solution:

The given problem will solve by using Avogadro number.

"It is the number of atoms , ions and molecules in one gram atom of element, one gram molecules of compound and one gram ions of a substance". The number 6.022 × 10²³ is called Avogadro number.

Moles of oxygen:

1 mole = 6.022 × 10²³ molecules

3.01 × 10²² molecules × 1 mol / 6.022 × 10²³ molecules

0.05 moles of O₂

Number of atoms of oxygen:

1 mole = 6.022 × 10²³ atoms

0.05 mol × 6.022 × 10²³ atoms /1 mol

0.3× 10²³ atoms of oxygen

Volume of oxygen:

1 mole of oxygen at STP occupy 22.414 dm³

0.05 mol × 22.414 dm³ / 1mol

1.1207 dm³

Mass of oxygen:

Mass = number of moles × molar mass

Mass = 0.05 mol × 32 g/mol

Mass = 1.6 g

8 0

3 years ago

Which of the following statements about boiling points is true?

lutik1710 [3]

<span>The boiling point of a substance is higher than its freezing point</span>

5 0

3 years ago