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asambeis [7]
3 years ago
13

How much CO2 is produced from 10g of CH4?

Chemistry
1 answer:
prohojiy [21]3 years ago
3 0

Answer:

0.625 moles of CO₂ can be produced by this reaction.

27.5 g of CO₂

Explanation:

A reaction where CO₂ can be produced is combustion.

The reactants are methane (in this case) and oxygen, while the products will be CO₂ and  H₂O.

The balanced reaction is: CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g)

We assume the oxygen is in excess, so the methane gas, is the limiting reagent.

We convert the mass to moles (mass / molar mass) → 10 g / 16 g/mol = 0.625 moles

According to stoichiometry, 1 mol of methane can produce 1 mol of CO₂. Therefore If we have 0.625 moles of CH₄ we produce 0.625 moles of CO₂. Ratio is 1:1.

Let's convert the moles to mass → (mol . molar mass) =

0.625 mol . 44 g/mol = 27.5 g

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Does water added to a flask containing chlorine gas and solid sodium react in the chemical reaction to make sodium chloride
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1 year ago
how many moles of silicon are in 245 g of silicon? a. 8.72 mol b. 28.0 mol c. 1.10 × 10-1 mol d. 6.90 × 103 mol
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A gas has a volume of 62.65L at O degrees Celsius and 1 atm. At what temperature in Celsius would the volume of the gas be 78.31
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Answer:

The volume of the gas will be 78.31 L at 1.7 °C.

Explanation:

We can find the temperature of the gas by the ideal gas law equation:

PV = nRT

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n: is the number of moles

V: is the volume

T: is the temperature

R: is the gas constant = 0.082 L*atm/(K*mol)

From the initial we can find the number of moles:

n = \frac{P_{1}V_{1}}{RT_{1}} = \frac{1 atm*62.65 L}{(0.082 L*atm/K*mol)*(0 + 273)K} = 2.80 moles

Now, we can find the temperature with the final conditions:

T_{2} = \frac{P_{2}V_{2}}{nR} = \frac{612.0 mmHg*\frac{1 atm}{760 mmHg}*78.31 L}{2.80 moles*0.082 L*atm/(K*mol)} = 274.7 K

The temperature in Celsius is:

T_{2} = 274.7 - 273 = 1.7 ^{\circ} C

Therefore, the volume of the gas will be 78.31 L at 1.7 °C.

I hope it helps you!            

8 0
3 years ago
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