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3 years ago

11

Cu2o+C➡Cu+Co2 what is the balance chemical equation

1 answer:

denis23 [38]3 years ago

5 0

<span>4 Cu2O + C2 = 8 Cu + 2 CO2 </span><span>Reaction type: single replacement i hope this hopes

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The following balanced equation shows the decomposition of ammonia (NH3) into nitrogen (N2) and hydrogen (H2). 2NH3 → N2 + 3H2 A

Triss [41]

The decomposition of ammonia is characterized by the following decomposition equation:
2NH₃<span> → N</span>₂ <span> + 3H</span>₂

The mole ratio of N₂ : H₂ is 1 : 3

If the number of moles of N₂ = 0.0351 mol
Then the number of moles of H₂ = 0.0351 mol × 3
= 0.1053 mol

The number of moles of hydrogen gas produced when 0.0351 mol of Nitrogen gas is produced after the decomposition of Ammonia is 0.105 mol (OPTION 3).

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3 years ago

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Water droplets forming on the inside of a cold windshield is an example of

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Condensation I think.

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3 years ago

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Various members of a class of compounds, alkenes, react with hydrogen to produce a corresponding alkane. Termed hydrogenation, t

Vitek1552 [10]

<u>Answer:</u> The mass of decane produced is $1.743\times 10^2g$

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ......(1)

Mass of hydrogen gas = 2.45 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1:, we get:

$\text{Moles of }H_2=\frac{2.45g}{2g/mol}=1.225mol$

The chemical equation for the hydrogenation of decene follows:

$C_{10}H_{20}(l)+H_2(g)\rightarrow C_{10}H_{22}(s)$

As, decene is present in excess. So, it is considered as an excess reagent.

Thus, hydrogen gas is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of hydrogen gas produces 1 mole of decane.

So, 1.225 moles of hydrogen gas will produce = $\frac{1}{1}\times 1.225=1.225mol$ of decane

Now, calculating the mass of decane by using equation 1, we get:

Moles of decane = 1.225 mol

Molar mass of decane = 142.30 g/mol

Putting values in equation 1, we get:

$1.225mol=\frac{\text{Mass of decane}}{142.30g/mol}\\\\\text{Mass of carbon dioxide}=(1.225mol\times 142.30g/mol)=174.3g=1.743\times 10^2g$

Hence, the mass of decane produced is $1.743\times 10^2g$

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3 years ago

To prevent poisoning, what three items should NEVER be taken into the lab?

Roman55 [17]

The answer of this answer is given in the attached file

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3 years ago

A ball was kicked by a player, the ball was stationary, then it gains a velocity of 5 m/s North. Did the ball accelerate or no?

Tomtit [17]

Answer:

yes

Explanation:

it started moving North 5 m/s

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3 years ago