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xxMikexx [17]
2 years ago
9

Click here to access the interactive simulation. You will practice balancing chemical equations by playing an interactive game.

After accessing the website, select the game box and start with level 1, followed by levels 2 and 3. The goal of these games is to have the same number of atoms on each side of the equation.
In level 1, you balanced the equation N2 + H2 →

NH3. What number did you place in front of ammonia (NH3)?

In level 2, you balanced the equation C + H2O → CH4 +

CO2. What number did you place in front of carbon dioxide (CO2)?

In level 3, you balanced the equation NH3 + O2 → NO2 +
H2O. What number did you place in front of water?
Chemistry
1 answer:
Mice21 [21]2 years ago
7 0

Answer:

In level 1, you balanced the equation N2 + H2 →  

✔ 2

NH3. What number did you place in front of ammonia (NH3)?

In level 2, you balanced the equation C + H2O → CH4 +  

✔ 1

CO2. What number did you place in front of carbon dioxide (CO2)?

In level 3, you balanced the equation NH3 + O2 → NO2 +  

✔ 6

H2O. What number did you place in front of water?

Explanation:

Edge:2020

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3 Ni2+(aq) + 2 Cr(OH)3(s) + 10 OH− (aq) → 3 Ni(s) + 2 CrO42−(aq) + 8 H2O(l) ΔG∘ = +87 kJ/molGiven the standard reduction potenti
Mrrafil [7]

Answer:

The standard reduction potential E°cell (Cr6+/Cr3+) is -0.13V

Explanation:

<u>Step 1</u>: Data given

3 Ni^2+(aq) + 2 Cr(OH)3(s) + 10 OH− (aq) → 3 Ni(s) + 2 CrO4^2−(aq) + 8 H2O(l) ΔG∘ = +87000 J/mol

Ni2+(aq) + 2 e− → Ni(s)    E∘red = -0.28 V

<u>Step 2:</u> The half reactions:

Cathode:  Ni2+(aq) + 2 e− → Ni(s)    E° = -0.28 V

Anode: CrO4^2-(aq) + 4H2O(l) +3e- → Cr(OH)3(s) + 5OH- (aq)   E°= unknown

<u>Step 3:</u> Calculate E°cell

ΔG° = -n*F*E°cell

⇒ with ΔG° = the gibbs free energy

⇒ n = the number of electrons in the net reaction = 6

⇒ F = the Faraday constant = 96485 C

⇒ E°cell= the standard cell potential

<u>Step 4:</u> Calculate E°(Cr6+/Cr3+

E°cell= ΔG°/(-n*F)

E°cell = 87000 /(-6*96485)

E°cell = -0.150 V

E°cell = E°(Ni2+/Ni) - E°(Cr6+/Cr3+)

E°(Cr6+/Cr3+) = -0.13V

The standard reduction potential E°cell (Cr6+/Cr3+) is -0.13V

7 0
2 years ago
A 12.2-g sample of x reacts with a sample of y to form 78.9 g of xy. what is the mass of y that reacted?
Sonja [21]
We will assume that the only reactants are x and y and that the only product is xy.

Based on the law of mass conservation, mass is an isolated system that can neither be created nor destroyed.

Applying this concept to the chemical reaction, we will find that the total mass of the reactants must be equal to the total mass of the products,
therefore:
mass of x + mass of y = mass of xy
12.2 + mass of y = 78.9
mass of y = 78.9 - 12.2 = 66.7 grams
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I did the math on a calculator and it was the closest atomic mass to potassium.

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