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garik1379 [7]
3 years ago
5

It has been estimated that 8.0 x 10^4 tons of gold (Au) have been mined. Assume gold costs $1350 per troy ounce. What is the tot

al worth of this quantity of gold? (1 troy ounce =31.103 g)
Chemistry
1 answer:
vodomira [7]3 years ago
4 0

Answer:

\$ 3.14\times 10^{12} is the total worth of this quantity of gold.

Explanation:

Estimated mass of gold =M = 8.0\times 10^4 tons

1 troy ounce = 31.103 g

1 ton = 907185 g

1 g= \frac{1}{907185} ton

31.103 g= 31.103\times \frac{1}{907185} ton=3.4285\times 10^{-5} ton

1 troy ounce =3.4285\times 10^{-5}ton

1 ton = \frac{1}{3.4285\times 10^{-5}}\text{troy ounce}

=2.9167\times 10^4 \text{troy ounce}

M = 8.0\times 10^4 tons=8.0\times 10^4\times 2.9167\times 10^4 \text{troy ounce}

M = 2.333\times 10^{9} troy ounces

Cost of 1 troy ounce gold = $1350

Cost of  2.333\times 10^{9} troy ounces of gold =

\$1350\times 2.333\times 10^{9} =\$ 3.14\times 10^{12}

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Complete and balance the following redox equation using the set of smallest whole– number coefficients. Now sum the coefficients
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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)

The sum of the coefficients is, 17

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

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

The balanced chemical equation in acidic medium will be,

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

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

The sum of the coefficients = 17

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