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3 years ago

PLEASE HELP ASAP

Chemistry

1 answer:

snow_lady [41]3 years ago

8 0

Answer:

See explanation

Explanation:

A redox reaction equation shows a gain/loss of electrons from left to right in a reaction. In a redox reaction, a specie looses electrons while another specie gains electrons.

Considering the equation; 2Al(s) + 3Cu(NO3)2(aq) -----> 3Cu(s) + 2Al(NO3)3(aq)

The oxidation state of Al reactant is zero since the oxidation state of all uncombined elements is zero. The oxidation state of All in the product is +3

The oxidation state of the copper in the reactant is +2. The oxidation state of copper in the product is zero.

The oxidation state of N in the reactant and product is +5.

The oxidation state of oxygen in the reactant and product is (-2).

This is a redox reaction because from left to right, Al was oxidized (oxidation number increased from zero to +3) while Cu was reduced (oxidation number decreased from +2 to zero).

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Im to lazy to do this.

san4es73 [151]

D is correct answer

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3 years ago

Which has a greater volume, 10 grams of water or 10 grams of acetone?

WINSTONCH [101]

Density is defined as the ratio of mass to the volume.

Density = $\frac{Mass}{Volume}$ (1)

Mass of water = 10 grams

Mass of acetone = 10 grams

Density of water = 1 $\frac{g}{cm^{3}}$

Density of acetone = 0.7857 $\frac{g}{cm^{3}}$

Put the value of density of water and its mass in equation (1)

1 $\frac{g}{cm^{3}}$ = $\frac{10 g}{volume}$

Volume of water = 10 $cm^{3}$

Put the value of density of acetone and its mass in equation (1)

0.7857 $\frac{g}{cm^{3}}$ = $\frac{10 g}{volume}$

Volume of acetone = 12.72 $cm^{3}$

Thus, volume of acetone is more than volume of water because the density of acetone is lower.

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3 years ago

8.0 mol AgNO3 reacts with 5.0 mol Zn in

Yakvenalex [24]

Taking into account the reaction stoichiometry, 8 moles of Ag can be produced from 8 moles of AgNO₃ and 5 moles of Zn.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

2 AgNO₃ + Zn → 2 Ag + Zn(NO₃)₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

AgNO₃: 2 moles
Zn: 1 mole
Ag: 2 moles
Zn(NO₃)₂: 1 mole

<h3>Limiting reagent</h3>

The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.

<h3>Limiting reagent in this case</h3>

To determine the limiting reagent, it is possible to use a simple rule of three as follows: if by stoichiometry 1 mole of Zn reacts with 2 moles of AgNO₃, 5 moles of Zn reacts with how many moles of AgNO₃?

$amount of moles of AgNO_{3}= \frac{5 moles of Znx2 moles of AgNO_{3}}{1 mole of Zn}$

<u><em>amount of moles of AgNO₃= 10 moles </em></u>

But 10 moles of AgNO₃ are not available, 8 moles are available. Since you have less moles than you need to react with 5 moles of Zn, AgNO₃ will be the limiting reagent.

<h3>Moles of Ag formed</h3>

Considering the limiting reagent, the following rule of three can be applied: if by reaction stoichiometry 2 moles of AgNO₃ form 2 moles of Ag, 8 moles of AgNO₃ form how many moles of Ag?

$amount of moles of Ag=\frac{8 moles of AgNO_{3}x2 moles of Ag }{2 moles of AgNO_{3}}$

<u><em>amount of moles of Ag= 8 moles</em></u>

Then, 8 moles of Ag can be produced from 8 moles of AgNO₃ and 5 moles of Zn.

Learn more about the reaction stoichiometry:

<u>brainly.com/question/24741074</u>

<u>brainly.com/question/24653699</u>

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2 years ago

What happens when an island volcano erupts and molten lava flows out?

qwelly [4]

It will explode together cause danger

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3 years ago

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A student weighs out 0. 0422 g of magnesium metal. The magnesium metal is reacted with excess hydrochloric acid to produce hydro

lutik1710 [3]

The student weighs out 0.0422 grams of the metal magnesium, thus we can figure that the more's, the magnesium he used, is the mass of the magnesium over the more mass, which is 0.024422.
That is approximately 0.001758.
Furthermore, it claims that too much hydrochloric acid causes the metal magnesium to react, producing hydrogen gas.
The volume of collected gas is 43.9 cc, the mastic pressure is 22 cc, and a sample of hydrogen gas is collected over water in a meter.

<h3>Is it true that calculations made utilizing experimental and gathered data result in a percent error? </h3>

Consequently, we are aware that magnesium and chloride react.
We create 1 as the reaction ratio is 1:2.
The hydrogen and 1 are more.
Magnesium chloride is more.
Therefore, based on this equation, we can infer that the amount of hydrogen that would be created in this scenario is greater than the amount of magnesium present here, or 0.001758 more.
Among hydrogen, there is.
\Once we convert the temperature from 32 Celsius to kelvin, we can tell you that the temperature is actually about 5.15 kelvin.
The gas has a volume of 43 in m, which is equal to 0.0439 liter and indicates that the pressure is approximately 832 millimeter.
Mercury, which is 2 times 13332 plus ca, or roughly 110922.24 par, is a mathematical constant.
So, in this instance, we are aware that p v = n r t.
The r in this case equals p v over n t, thus we want to determine the r.
So p is 110922.24. The temperature is 305.15 and the V is 0.04 over the n is 0.001758.
Let's proceed with the calculations right now.
In this instance, you will discover that the solution is 9.077 times 10; that is all there is to it.

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2 years ago