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3 years ago

I need what kind of energy is number two

Chemistry

2 answers:

Thepotemich [5.8K]3 years ago

4 0

<u>answers:</u>

- electrical (using power), sound (tv making noise), light (tv making colors for darrick to see), and some heat energy

-potential (when stopping on top of the ramp), kinetic (when riding down the ramp), mechanical (the skateboard).

hope this helps!❤from peachimin

Ilya [14]3 years ago

3 0

Electrical energyI'm pretty sure the answer would be electerical energy

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katovenus [111]

Answer:

2Fe⁺³ + Sn₂ → 2Fe⁺² + 2Sn⁺²

Explanation:

A redox reaction occurs between a compound that loses electrons and others that gain an electron. The first is being oxidized, and the other is being reduced.

In this situation, in the compound Fe₂O₃, the iron, has an oxidation number equal to +3, so it's Fe⁺³, and it will gain 1 electron to become Fe⁺². Because it was first dissolved in HCl, we must use the ion at the equation. The other compound Sn₂ will be oxidized to Sn⁺², so it will need to lose 2 electrons.

So, it will be necessary 2 Fe⁺³ for this reaction happen:

2Fe⁺³ + Sn₂ → 2Fe⁺² + 2Sn⁺²

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3 years ago

Suppose of barium acetate is dissolved in of a aqueous solution of ammonium sulfate. Calculate the final molarity of barium cati

ollegr [7]

Explanation:

Let us assume that the given data is as follows.

mass of barium acetate = 2.19 g

volume = 150 ml = 0.150 L (as 1 L = 1000 ml)

concentration of the aqueous solution = 0.10 M

Therefore, the reaction equation will be as follows.

$Ba(C_{2}H_{3}O_{2})_{2} \rightarrow Ba^{2+} + 2C_{2}H_{3}O^{-}_{2}$

Hence, moles of $C_{2}H_{3}O^{-}_{2}$ = $2 \times Ba(C_{2}H_{3}O_{2})_{2}$ .......... (1)

As, No. of moles = $\frac{mass}{\text{molar mass}}$

Hence, moles of $Ba(C_{2}H_{3}O_{2})_{2}$ will be calculated as follows.

No. of moles = $\frac{mass}{\text{molar mass}}$

= $\frac{2.19 g}{255.415 g/mol}$ (molar mass of $Ba(C_{2}H_{3}O_{2})_{2}$ is 255.415 g/mol)

= $8.57 \times 10^{-3}$

Moles of $C_{2}H_{3}O^{-}_{2}$ = $2 \times 8.57 \times 10^{-3}$

= 0.01715 mol

Hence, final molarity will be as follows.

Molarity = $\frac{\text{no. of moles}}{volume}$

= $\frac{0.01715 mol}{0.150 L}$

= 0.114 M

Thus, we can conclude that final molarity of barium cation in the solution is 0.114 M.

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Answer:

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$NH_3+HNO_3-> NH_4NO_3$

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So, number of moles of nitric acid required are also 62500 moles.

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