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kolezko [41]
2 years ago
11

Hurry please!

Chemistry
1 answer:
Pani-rosa [81]2 years ago
5 0

Answer : The mass of of water present in the jar is, 298.79 g

Solution : Given,

Mass of barium nitrate = 27 g

The solubility of barium nitrate at 20^oC is 9.02 gram per 100 ml of water.

As, 9.02 gram of barium nitrate present in 100 ml of water

So, 27 gram of barium nitrate present in \frac{27g}{9.02g}\times 100ml=299.33ml of water

The volume of water is 299.33 ml.

As we know that the density of water at 20^oC is 0.9982 g/ml

Now we have to calculate the mass of water.

\text{Mass of water}=\text{Density of water}\times \text{Volume of water}

\text{Mass of water}=(0.9982g/ml)\times (299.33ml)=298.79g

Therefore, the mass of of water present in the jar is, 298.79 g

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We have 1700 Tonnes of Amoniac every day. How many tonnes of 63% Nitrogen soda we can get?
V125BC [204]
There are 3 equations involved in manufacturing Nitric Acid from Ammonia. 

First the ammonia is oxidized:
4NH3 + 5O2 = 4NO + 6H2O

Then for the absorption of the nitrogen oxides.
2NO + O2 = N2O4

Lastly, the N2O4 is further oxidized into Nitric acid.
3N2O4 + 2H2O = 4HNO3 + 2NO

Then run stoichiometry through these equations.
The first equation produces roughly 271,722,938 grams of NO
The second equation produces roughly 416,606,944 grams of N2O4
The last equation produces roughly 380,412,294 grams of HNO3 (nitric acid)

Convert the exact number back into tons, and your answer is: 419.332775 tons.

Rounded, I'm going to say that's 419.33 tons.
Hope this helps! :)

Also, it seems that commercially, Nitric Acid is commonly made by bubbling NO2 into water, rather than using ammonia.
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3 years ago
Which of thes is a property of a substance that is composed of atoms that are held together by ionic bonds?
Svetlanka [38]

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Which type of salt would be most effective for melting ice on roads?
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Calculate for the following electrochemical cell at 25°C, Pt H2(g) (1.0 atm) H (0.010 M || Ag (0.020 M) Ag if E (H) - +0.000 V a
viva [34]

Answer : The correct option is, (b) +0.799 V

Solution :

The values of standard reduction electrode potential of the cell are:

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E^0_{[Ag^{+}/Ag]}=+0.799V

From the cell representation we conclude that, the hydrogen (H) undergoes oxidation by loss of electrons and thus act as anode. Silver (Ag) undergoes reduction by gain of electrons and thus act as cathode.

The half reaction will be:

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Reaction at cathode (reduction) : Ag^{+}+1e^-\rightarrow Ag    

The balanced cell reaction will be,  

H_2+2Ag^{+}\rightarrow 2H^{+}+2Ag

Now we have to calculate the standard electrode potential of the cell.

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E^o_{cell}=E^o_{[Ag^{+}/Ag]}-E^o_{[H^{+}/H_2]}

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Therefore, the standard cell potential will be +0.799 V

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The response would become spontaneous if the value of  ΔG° was negative.

According to the estimated value of  ΔG°, it is shown that  ΔG° value decreases as temperature value increases. The value shifts from being more favorable to being less favorable. It would appear that the value of  ΔG° would be negative at a specific temperature, causing the reaction to occur spontaneously.

The reaction is in an equilibrium state if  ΔG = 0. If ΔG < 0, the reaction is spontaneous in the direction written. The relationship between terms from the equilibrium is paralleled by the relevance of the sign of a change in the Gibbs free energy.

Learn more about ΔG° here:

brainly.com/question/14512088

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