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sergij07 [2.7K]
3 years ago
12

How much energy is released when 22.4g of CH4 is burned?

Chemistry
1 answer:
solniwko [45]3 years ago
5 0

The combustion of methane, CH4, releases 890.4 kJ/mol. That is, when one mole of methane is burned, 890.4 kJ are given off to the surroundings. This means that the products have 890.4 kJ less than the reactants.

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Only oppositely charged objects can attract each other. true false
Delicious77 [7]
No as neutral object will attract and be attracted by a positive and negative charge 

hope that helps 
4 0
3 years ago
Can an intermediate appear as a reactant in the first step of a reaction mechanism?.
saveliy_v [14]

Answer:

No

Explanation:

An intermetiate in a chemical reaction is something that is formed and reused in a reaction.

8 0
2 years ago
Check wether all the answers are correct or not. please?​
zhenek [66]

Answer:

I dont now but I think it is correct

3 0
2 years ago
Read 2 more answers
In the following reaction, what is the quantity of heat (in kJ) released when 5.87 moles of CH₄ are burned?
IRISSAK [1]

Taking into account the definition of enthalpy of a chemical reaction, the quantity of heat released when 5.87 moles of CH₄ are burned is 4,707.74 kJ.

The enthalpy of a chemical reaction as the heat absorbed or released in a chemical reaction when it occurs at constant pressure. That is, the heat of reaction is the energy that is released or absorbed when chemicals are transformed into a chemical reaction.

The enthalpy is an extensive property, that is, it depends on the amount of matter present.

In this case, the balanced reaction is:

CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g)

and the enthalpy reaction ∆H° has a value of -802 kJ/mol.

This equation indicates that when 1 mole of CH₄ reacts with 2 moles of O2, 802 kJ of heat is released.

When 5.87 moles of CH₄ are burned, then you can apply the following rule of three: if 1 mole of CH₄ releases 802 kJ of heat, 5.87 moles of CH₄ releases how much heat?

heat=\frac{5.87 molesof CH_{4}x802 kJ}{1 mol of CH_{4} }

<u><em>heat= 4,707.74 kJ</em></u>

Finally, the quantity of heat released when 5.87 moles of CH₄ are burned is 4,707.74 kJ.

Learn more:

  • brainly.com/question/15355361?referrer=searchResults
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  • brainly.com/question/13813185?referrer=searchResults
  • brainly.com/question/19521752
5 0
2 years ago
A 0.055 mol sample of formaldehyde vapor, CH2O, was placed in a heated 500 mL vessel and some of it decomposed. The reaction is
Elis [28]

Answer:

Kc for this reaction is 0.06825

Explanation:

Step 1: Data given

Number of moles formaldehyde CH2O = 0.055 moles

Volume = 500 mL = 0.500 L

At equilibrium, the CH2O(g) concentration = 0.051 mol

Step 2: The balanced equation

CH2O  <=>  H2 + CO

Step 3: Calculate the initial concentrations

Concentration = moles / volume

[CH2O] = 0.055 moles . 0.500 L

[CH2O] = 0.11 M

[H2] = 0M

[CO] = 0M

Step 4: The concentration at the equilibrium

[CH2O] = 0.11 - X M = 0.051 M

[H2] = XM

[CO] = XM

[CH2O] = 0.11 - X M = 0.051 M

X = 0.11 - 0.051 = 0.059

[H2] = XM = 0.059 M

[CO] = XM = 0.059 M

Step 5: Calculate Kc

Kc = [H2][CO]/[CHO]

Kc = (0.059 * 0.059) / 0.051

Kc = 0.06825

Kc for this reaction is 0.06825

7 0
3 years ago
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