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Vedmedyk [2.9K]
3 years ago
7

Coke is an impure form of carbon that is often used in the in- dustrial production of metals from their oxides. If a sample of c

oke is 95% carbon by mass, determine the mass of coke needed to react completely with 1.0 ton of copper(II) oxide.
Chemistry
1 answer:
steposvetlana [31]3 years ago
3 0

Answer:

The mass of coke needed to react completely with 1.0 ton of copper(II) oxide is 0.794 Ton.

Explanation:

2CuO+C\rightarrow 2Cu+CO_2

1 Ton = 907185 grams

Mass of copper oxide = 1.0 Ton = 907185 grams

Moles of copper oxide =\frac{907185 g}{79.55 g/mol}=11,403.95 moles

According to reaction, 2 moles of copper oxide reacts with 1 mole of carbon.

Then 11403.95 moles of copper oxide will react with:

\frac{1}{2}\times 11403.95 mol=5,701.98 mol of carbon

Mass of 5,701.98 moles of carbon:

5,701.98 mol\times 12 g/mol=68,423.75 g

Mass of coke = x

Mass of carbon = 68,423.75 g

Percentage of carbon in coke = 95%

95\%=\frac{68,423.75 g}{x}\times 100

x=720,250.09 g=0.794 Ton

The mass of coke needed to react completely with 1.0 ton of copper(II) oxide is 0.794 Ton.

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Answer:

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Explanation:

<u>Question 1</u>

NaHCO3 + CH3COOH --> NaCH3COO + H2O + CO2

<em>To balance the equation, count the number of atoms on both sides of the equation</em>

(1 Na, 1+3+1H, 1+1+1C, 3+2Oxygen) --> (1 Na, 1+1+1C, 3+2H, 2+1+2Oxygen)

<em>Combining the pluses will give you the following</em>

(1 Na, 5H, 3C, 5Oxygen) --> (1 Na, 3C, 5H, 5Oxygen)

<em>Both sides are the same, therefore the chemical equation is balanced (originally). </em>

From the equation, we can see that <u>1 mole of NaHCO3</u> produces <u>1 mole of CO2</u>.

So that means <u>0.5 mole of NaHCO3</u> would produce <u>0.5 mole of CO2</u>.

<u>Question 2</u>

C4H10 + O2 --> CO2 + H2O

<em>Again, count the number of atoms on both sides of the equation</em>

(4C, 10H, 2O) --> (1C, 2H, 3O)     <em>This time left does not equal right side</em>

<em>You now need to find </em><u><em>factors </em></u><em>that can make both sides equal. </em>

C4H10 + O2 --> <u>4</u>CO2 + H2O    <em>Now the C is balanced, let's recount </em>

<em>(4C, 10H, 2Oxygen) --> (4C, 8+1Oxygen, 2H)      H&O is still not balanced</em>

C4H10 + O2 --> 4CO2 + <u>5</u>H2O    <em>Now the H is balanced, let's recount</em>

<em>(4C, 10H, 2Oxygen) --> (4C, 8+5Oxygen, 10H)      O is still not balanced</em>

C4H10 + (<u>13/2</u>)O2 --> 4CO2 + 5H2O    <em>Now the O is balanced</em>

<em>(4C, 10H, 13Oxygen) --> (4C, 13Oxygen, 10H)</em>

<em>But because 13/2 is a fraction, we want to eliminate that by multiplying every reactant and product by 2 (the denominator).</em>

<u>2</u>C4H10 + <u>13</u>O2 --> <u>8</u>CO2 + <u>10</u>H2O    Now it's completely balanced!

<em>(8C, 20H, 28Oxygen) --> (8C, 28Oxygen, 20H)     Yayy! It's balanced.</em>

Now, 2 mol C4H10 produces 8 mol CO2.

So 1 mol C4H10 produces 4 mol CO2.

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