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2 years ago

14

help, Look at the model below. Explain what is correct and/or incorrect about the model based on scale, proportion, and quantity

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1 answer:

stiks02 [169]2 years ago

6 0

One correct thging is that there are the same amount of positive and negative atoms

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A reaction is exothermic when Group of answer choices weak bonds break and strong bonds form. strong bonds break and weak bonds

Leona [35]

Answer:

weak bonds break and strong bonds form

Explanation:

An exothermic reaction is a chemical reaction in which heat energy is evolved during the reaction process.

Bond formation requires energy while bond breakage releases energy. More energy is needed for the formation of weak bonds as compared to strong bonds.

<em>Hence, when weak bonds break, they release more energy than needed to make a corresponding strong bond leading to the release of the remaining energy as heat.</em>

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3 years ago

C10H22 + O2 -- CO2 + H2O balance

Tasya [4]

Answer:

1,31÷2 =10,11

Explanation:

c10h22+31÷2o2=10co2+11h2o

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2 years ago

MgCl2 + AgNO3 → AgCl + Mg(NO3)2

Law Incorporation [45]

Answer:

MgCl2 + 2AgNO3 → 2AgCl + Mg(NO3)2

Explanation:

I'm assuming you want to balance it so...

The first thing I see is that there are two chlorines on the reactant side and one on the product side

Adding a coefficient of 2 would get 2AgCl2

Now there are two silvers on the reactant side, so add a 2 to AgNO3 on the products side. Now they are all balanced.

If that is not what you are looking for let me know!

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2 years ago

Read 2 more answers

What is Covalent bond?

Marina CMI [18]

<span>the sharing of electron pairs between atoms</span>

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3 years ago

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N2H4 + N2O4 --> N2 + H2O

ahrayia [7]

Answer:

The limiting reagent is N2O4
14,09g

Explanation:

First, we adjust the reaction.

$2N_{2} H_{4}$ + $N_{2} O_{4}$ ⇄ $6N_{2} + 4H_{2}O$

Second, we assume that the participating moles are equal to the stoichiometric ratios because we do not know the amounts of the reagents.

We can determinate what is the limiting reagent comparing of product amounts which can be formed from each reactant.

Using $N_{2} H_{4}$ to form $H_{2}O$

$molH_{2} O = 1mol N_{2} H_{4} } . \frac{4 mol H_{2} O}{2mol N_{2} H_{4} }. \frac{18\frac{g}{mol} H_{2} O}{1mol H_{2} O_} } . \frac{ 1 mol N_{2}H_{4} }{32,04\frac{g}{mol} N_{2} H_{4} }$

$molH_{2} O = 1, 125 mol$

Using $N_{2} O_{4}$ to form $H_{2} O$

$molH_{2} O = 1mol N_{2} O_{4} } . \frac{4 mol H_{2} O}{1mol N_{2} O_{4} }. \frac{18\frac{g}{mol} H_{2} O}{1mol H_{2} O_} } . \frac{ 1 mol N_{2}O_{4} }{92\frac{g}{mol} N_{2} O_{4} }$

$molH_{2} O = 0,783 mol$

The limiting reagent is N2O4, because can produce only 0, 783 mol of H2O.

This is the minimum measure can be formed of each product.

∴ $MassOfH_{2}O = 0,783mol . 18\frac{g}{mol}$

$MassOfH_{2}O = 14,09g$

5 0

3 years ago