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miss Akunina [59]

3 years ago

15

If you are mixing a solution in a spray bottle with 15 ounces of water, how much chlorine do you need to add for the correct rat

io?

1 answer:

Wittaler [7]3 years ago

7 0

15 ounces so you can make it even

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Identify the oxidized substance, the reduced substance, the oxidizing agent, and the reducing agent in the redox reaction. Cu(s)

spin [16.1K]

<u>Answer:</u> Copper is getting oxidized and is a reducing agent. Silver is getting reduced and is oxidizing agent.

<u>Explanation:</u>

Oxidation reaction is defined as the reaction in which an atom looses its electrons. Here, oxidation state of the atom increases.

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

Reduction reaction is defined as the reaction in which an atom gains electrons. Here, the oxidation state of the atom decreases.

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

Oxidizing agents are defined as the agents which oxidize other substance and itself gets reduced. These agents undergoes reduction reactions.

Reducing agents are defined as the agents which reduces the other substance and itself gets oxidized. These agents undergoes reduction reactions.

For the given chemical reaction:

$Cu(s)+2AgNO_3(aq.)\rightarrow 2Ag(s)+Cu(NO_3)_2(aq.)$

The half reactions for the above reaction are:

<u>Oxidation half reaction:</u> $Cu(s)\rightarrow Cu^{2+}(aq.)+2e^-$

<u>Reduction half reaction:</u> $2Ag^+(aq.)+2e^-\rightarrow 2Ag(s)$

From the above reactions, copper is loosing its electrons. Thus, it is getting oxidized and is considered as a reducing agent.

Silver is gaining electrons and thus is getting reduced and is considered as an oxidizing agent.

4 0

3 years ago

why do you think you can find silver and gold on their own in rocks but calcium and magnesium are combined with other elements t

katrin [286]

Explanation:

Silver and Gold belong to a special group of metals known as the native metals. They are found naturally on their own and not in combined form in rocks.

These metals are found uncombined because they are unreactive.
They prefer to alloy with themselves.
Calcium and magnesium on the other hand are reactive metals.
The unreactivity of these metals makes them uncombined in nature.

4 0

3 years ago

Read 2 more answers

If 1 kg of fuel is used in the above fusion reaction (2 1H + 3 1H--> 4 2He+1 0N) , the resulting helium has a mass of 0.993 k

enot [183]

Δmc
2

For one reaction:
Mass Defect =Δm
=2(m
H

)−m
He

−m
n

=2(2.015)−3.017−1.009
=0.004 amu
1 amu=931.5 MeV/c
2

Hence,
E=0.004×931.5 MeV=3.724 MeV
E=3.726×1.6×10
−13
J=5.96×10
−13
J

For 1 kg of Deuterium available,
moles=
2g
1000g

=500
N=500N
A

=3.01×10
26

Energy released =
2
N

×5.95×10
−13
J
=8.95×10
13

6 0

3 years ago

How reactive is an atom of Sodium(Na) and why?

s344n2d4d5 [400]

3rd one:
it is very reactive because it does not have a full Valence shell.

this is because it's in group 1 so it has one electron in its outer shell, and it wants to have a full outer shell ( which it can gain by losing the electron in a reaction).

Hope this helps :)

5 0

3 years ago

Aspirin sun thesis Green Chemistry and Assime the aspirin is prepared by the following reaction and that 10.09. of salicylic aci

klemol [59]

<u>Answer:</u> The percentage yield of aspirin is 38.02 %.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

<u>For salicylic acid:</u>

Given mass of salicylic acid $(C_7H_6O_3)$ = 10.09 g

Molar mass of salicylic acid $(C_7H_6O_3)$ = 138.12 g/mol

Putting values in equation 1, we get:

$\text{Moles of salicylic acid}=\frac{10.09g}{138.12g/mol}=0.0730mol$

The chemical equation for the formation of aspirin follows:

$C_7H_6O_3+C_4H_6O_3\rightarrow C_9H_8O_4+CH_3COOH$

As, acetic anhydride is present in excess. So, it is considered as an excess reagent.

Thus, salicylic acid is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin.

So, 0.0730 moles of salicylic acid will produce = $\frac{1}{1}\times 0.0730=0.0730mol$ of aspirin

Now, calculating the mass of aspirin from equation 1, we get:

Molar mass of aspirin = 180.16 g/mol

Moles of aspirin = 0.073 moles

Putting values in equation 1, we get:

$0.073mol=\frac{\text{Mass of aspirin}}{180.16g/mol}\\\\\text{Mass of aspirin}=13.15g$

To calculate the percentage yield of aspirin, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of aspirin = 5.0 g

Theoretical yield of aspirin = 13.15 g

Putting values in above equation, we get:

$\%\text{ yield of aspirin}=\frac{5.0g}{13.15g}\times 100\\\\\% \text{yield of aspirin}=38.02\%$

Hence, the percent yield of aspirin is 38.01 %.

6 0

3 years ago