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Aleonysh [2.5K]
3 years ago
9

How many centimeters are in 1 mile? Use the equalities 1 mile = 5280 feet; 1 foot = 12 inches; and 1 centimeter = 0.394 inches.

A. (5280 x 12 ∕ 0.394) cm B. 5280 ∕ (12 x 0.394) cm C. 5280 x 12 x 0.394 cm D. (5280 + 12 + 0.394) cm
Chemistry
2 answers:
Galina-37 [17]3 years ago
7 0
The answer is A which comes out to about 160812 cm
Alla [95]3 years ago
4 0

Answer:

A. \frac{5280*12}{0.394}cm

Explanation:

1. Take the quantity you want to convert:

1mile

2. Multiply by the first conversion factor:

1mile*\frac{5280feet}{1mile}

3. Apply the second conversion factor:

1mile*\frac{5280feet}{1mile}*\frac{12inches}{1foot}

4. Multiply by the third conversion factor:

1mile*\frac{5280feet}{1mile}*\frac{12inches}{1foot}*\frac{1centimeter}{0.394inches}

5. Multiply all the numerators and divide by denominators:

1mile*\frac{5280feet}{1mile}*\frac{12inches}{1foot}*\frac{1centimeter}{0.394inches}=\frac{5280*12}{0.394}cm

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Answer : The balanced chemical equation in a acidic solution is,

BrO_3^-(aq)+6H^+(aq)+3Sb^{3+}(aq)\rightarrow Br^-(aq)+3H_2O(l)+3Sb^{5+}(aq)

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Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

Rules for the balanced chemical equation in acidic solution are :

First we have to write into the two half-reactions.

Now balance the main atoms in the reaction.

Now balance the hydrogen and oxygen atoms on both the sides of the reaction.

If the oxygen atoms are not balanced on both the sides then adding water molecules at that side where the less number of oxygen are present.

If the hydrogen atoms are not balanced on both the sides then adding hydrogen ion (H^+) at that side where the less number of hydrogen are present.

Now balance the charge.

The given chemical reaction is,

BrO_3^-(aq)+Sb^{3+}(aq)\rightarrow Br^-(aq)+Sb^{5+}(aq)

The oxidation-reduction half reaction will be :

Oxidation : Sb^{3+}\rightarrow Sb^{5+}

Reduction : BrO_3^-\rightarrow Br^-

  • First balance the main element in the reaction.

Oxidation : Sb^{3+}\rightarrow Sb^{5+}

Reduction : BrO_3^-\rightarrow Br^-

  • Now balance oxygen atom on both side.

Oxidation : Sb^{3+}\rightarrow Sb^{5+}

Reduction : BrO_3^-\rightarrow Br^-+3H_2O

  • Now balance hydrogen atom on both side.

Oxidation : Sb^{3+}\rightarrow Sb^{5+}

Reduction : BrO_3^-+6H^+\rightarrow Br^-+3H_2O

  • Now balance the charge.

Oxidation : Sb^{3+}\rightarrow Sb^{5+}+2e^-

Reduction : BrO_3^-+6H^++6e^-\rightarrow Br^-+3H_2O

The charges are not balanced. Now multiplying oxidation reaction by 3 and then adding both equation, we get the balanced redox reaction.

Oxidation : 3Sb^{3+}\rightarrow 3Sb^{5+}+6e^-

Reduction : BrO_3^-+6H^++6e^-\rightarrow Br^-+3H_2O

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The sum of the coefficients = 1 + 6 + 3 + 1 + 3 + 3

The sum of the coefficients = 17

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