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kolbaska11 [484]
1 year ago
7

Zinc metal (Zn) will react with aqueous hydrochloric acid (HCI aq) to produce aqueous zinc chloride (ZnCl2 aq) and hydrogen gas

(H2). Which of the following isthe complete, balanced equation for this reaction?1. 2 HCI (aq) + 2 Zn (s) > 2 H2 (g) + ZnCl2 (aq)2. HCI (aq) + Zn (s) > H2 (g) + ZnCl2 (ag)3. 2 HCI (aq) + Zn (s) › 2 H2 (g) + ZnCl2 (ag)4. 2 HCI (aq) + Zn (s) › H2 (g) + 2 ZnCl2 (ag)5. 2 HCI (aq) + Zn (s) › H2 (g) + ZnCl2 (ad)
Chemistry
1 answer:
Debora [2.8K]1 year ago
3 0

Answer:

5

Explanation:

Here, we want to get the equation of the reaction between Hydrochloric acid and Zinc metal

Zinc metal displaces the hydrogen from hydrochloric acid to form zinc chloride

We have the equation of reaction as:

2HCl_{(aq)}\text{ + Zn}_{(s)}\text{ }\rightarrow\text{ ZnCl}_{2(aq)}\text{ + H}_{2(g)}

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koban [17]

Answer:

No, it is not sufficient

Please find the workings below

Explanation:

Using E = hf

Where;

E = energy of a photon (J)

h = Planck's constant (6.626 × 10^-34 J/s)

f = frequency

However, λ = v/f

f = v/λ

Where; λ = wavelength of light = 325nm = 325 × 10^-9m

v = speed of light (3 × 10^8 m/s)

Hence, E = hv/λ

E = 6.626 × 10^-34 × 3 × 10^8 ÷ 325 × 10^-9

E = 19.878 × 10^-26 ÷ 325 × 10^-9

E = 19.878/325 × 10^ (-26+9)

E = 0.061 × 10^-17

E = 6.1 × 10^-19J

Next, we work out the energy required to dissociate 1 mole of N=N. Since the bond energy is 418 kJ/mol.

E = 418 × 10³ ÷ 6.022 × 10^23

E = 69.412 × 10^(3-23)

E = 69.412 × 10^-20

E = 6.9412 × 10^-19J

6.9412 × 10^-19J is required to break one mole of N=N bond.

Based on the workings above, the photon, which has an energy of 6.1 × 10^-19J is not sufficient to break a N=N bond that has an energy of 6.9412 × 10^-19J

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