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Hatshy [7]
3 years ago
15

The buildings in this old mine are made of metal. You can see over 100 years, the silver color of the buildings has changed. The

red-brown color is rust. What does this color change tell us about the metal? A) The metal is malleable. B) The metal reacts in the presence of air and water. C) Acid rain has damaged the building over the years. D) The metal is a good conductor of heat and electricity.
Chemistry
2 answers:
Anna11 [10]3 years ago
8 0

Answer:

The correct answer is option B.

Explanation:

4Fe(s)+3O_2(g)\rightarrow 2Fe_2O_3(s)

Iron in presence of moisture reacts with oxygen gas to from iron(III) oxide of red brown color often termed as rust.

Building material used up in min building is metal which which span of time changed its color to rust formation. Therefore this means rust or change in color is due to the iron metal which reacts with oxygen and water present in the air.

vladimir2022 [97]3 years ago
5 0
The correct answer is:  [<span>B]:  "The metal reacts in the presence of air and water." 
____________________________________________________________</span>
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5

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2 years ago
The reaction described by H2(g)+I2(g)⟶2HI(g) has an experimentally determined rate law of rate=k[H2][I2] Some proposed mechanism
MatroZZZ [7]

Answer:

Mechanism A and B are consistent with observed rate law

Mechanism A is consistent with the observation of J. H. Sullivan

Explanation:

In a mechanism of a reaction, the rate is determinated by the slow step of the mechanism.

In the proposed mechanisms:

Mechanism A

(1) H2(g)+I2(g)→2HI(g)(one-step reaction)

Mechanism B

(1) I2(g)⇄2I(g)(fast, equilibrium)

(2) H2(g)+2I(g)→2HI(g) (slow)

Mechanism C

(1) I2(g) ⇄ 2I(g)(fast, equilibrium)

(2) I(g)+H2(g) ⇄ HI(g)+H(g) (slow)

(3) H(g)+I(g)→HI(g) (fast)

The rate laws are:

A: rate = k₁ [H2] [I2]

B: rate = k₂ [H2] [I]²

As:

K-1 [I]² = K1 [I2]:

rate = k' [H2] [I2]

<em>Where K' = K1 * K2</em>

C: rate = k₁ [H2] [I]

As:

K-1 [I]² = K1 [I2]:

rate = k' [H2] [I2]^1/2

Thus, just <em>mechanism A and B are consistent with observed rate law</em>

In the equilibrium of B, you can see the I-I bond is broken in a fast equilibrium (That means the rupture of the bond is not a determinating step in the reaction), but in mechanism A, the fast rupture of I-I bond could increase in a big way the rate of the reaction. Thus, just <em>mechanism A is consistent with the observation of J. H. Sullivan</em>

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3 years ago
What does fire mean​
Bond [772]

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Explanation:

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2 years ago
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<u>C Chemical Energy</u>

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At 350°c, keq = 1.67 × 10-2 for the reversible reaction 2hi (g) ⇌ h2 (g) + i2 (g). what is the concentration of hi at equilibriu
mariarad [96]
According to the reversible reaction equation:

2Hi(g) ↔ H2(g) + i2(g)

and when Keq is the concentration of the products / the concentration of the reactants.

Keq = [H2][i2]/[Hi]^2

when we have Keq = 1.67 x 10^-2

[H2] = 2.44 x 10^-3

[i2] = 7.18 x 10^-5

so, by substitution:

1.67 x 10^-2 = (2.44 x 10^-3)*(7.18x10^-5)/[Hi]^2

∴[Hi] = 0.0033 M
7 0
3 years ago
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