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3 years ago

Mass_mole relationship

Chemistry

1 answer:

gogolik [260]3 years ago

4 0

I mole equals mass in grams. There are 6.2*10^23 atoms per mole. Hope that helps

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Which is TRUE of the products in this combustion reaction? 4Fe + 3O2 2Fe2O3

ycow [4]

The only true answer is A.

products are on the right side of the reaction

products and reactants don't necessarily have same physical or chemical properties

It is the reactants that <span>are the atoms, molecules, or compounds that participate in the reaction.</span>

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3 years ago

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Emily spills concentrated sodium hydroxide solution on her lab bench. What she should do first?

blagie [28]

<h2>Answer:</h2>

She should notify her teacher.

<h2>Explanation:</h2>

Sodium Hydroxide is very corrosive in nature and it causes Redness, Pain, Serious skin burns and Blisters. Sodium hydroxide does not produce systemic toxicity, but is very CORROSIVE and can cause severe burns in all tissues that it comes in contact with. Therefore she should not touch it and she must notify her teacher as soon as possible.

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2 years ago

Consider the following reaction

Fynjy0 [20]

Answer:

92.72 kJ

Explanation:

2 N₂ (g) + O₂ (g) —-> 2 N₂O

According to question , one mole of N₂O requires 163.2 kJ of heat

Molecular weight of N₂O = 44 gm

25 g N₂O = 25 / 44 mole

25 / 44 mole will require 163.2 x 25 / 44 kJ

= 92.72 kJ

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2 years ago

Solid iron metal reacts with solid sulfur at room temperature to produce solid iron (ll) sulfide? Express as a chemical equation

kupik [55]

Answer:Fe+S=FeS

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2 years ago

Under standard-state conditions, which of the following species is the best reducing agent? a. Ag+ b. Pb c. H2 d. Ag e. Mg2+

eimsori [14]

<u>Answer:</u> The correct answer is Option b.

<u>Explanation:</u>

Reducing agents are defined as the agents which help the other substance to get reduced and itself gets oxidized. They undergo oxidation reaction.

$X\rightarrow X^{n+}+ne^-$

For determination of reducing agents, we will look at the oxidation potentials of the substance. Oxidation potentials can be determined by reversing the standard reduction potentials.

For the given options:

<u>Option a:</u> $Ag^+$

This ion cannot be further oxidized because +1 is the most stable oxidation state of silver.

<u>Option b:</u> $Pb$

This metal can easily get oxidized to $Pb^{2+}$ ion and the standard oxidation potential for this is 0.13 V

$Pb\rightarrow Pb^{2+}+2e^-;E^o_{(Pb/Pb^{2+})}=+0.13V$

<u>Option c:</u> $H_2$

This metal can easily get oxidized to $H^{+}$ ion and the standard oxidation potential for this is 0.0 V

$H_2\rightarrow 2H^++2e^-;E^o_{(H_2/H^{+})}=0.0V$

<u>Option d:</u> $Ag$

This metal can easily get oxidized to $Ag^{+}$ ion and the standard oxidation potential for this is -0.80 V

$Ag\rightarrow Ag^{+}+e^-;E^o_{(Ag/Ag^{+})}=-0.80V$

<u>Option e:</u> $Mg^{2+}$

This ion cannot be further oxidized because +2 is the most stable oxidation state of magnesium.

By looking at the standard oxidation potential of the substances, the substance having highest positive $E^o$ potential will always get oxidized and will undergo oxidation reaction. Thus, considered as strong reducing agent.

From the above values, the correct answer is Option b.

8 0

3 years ago