High School

For the reaction:

\[ \text{C (graphite)} + \text{O}_2 \rightarrow \text{CO}_2 \]

Given: \(\Delta H^\circ = -11020 \, \text{kJ/mol}\)

Calculate the released heat (kJ/mol) from burning 0.30 g of C (graphite).

Options:
A. -523
B. -44
C. +44
D. 275
E. -1.41%
F. 103

Answer :

Final answer:

The released heat from burning 0.30 g of carbon (graphite) is approximately -275.55 kJ/mol.

Explanation:

To calculate the released heat from burning 0.30 g of carbon (graphite), we need to follow these steps:

  1. Convert the given mass of carbon (graphite) to moles using its molar mass.
  2. Use the balanced chemical equation to determine the molar ratio between carbon (graphite) and carbon dioxide (CO2).
  3. Calculate the moles of carbon dioxide (CO2) produced.
  4. Finally, multiply the moles of carbon dioxide (CO2) by the enthalpy change (∆H) to calculate the released heat.

Step 1: Convert mass of carbon (graphite) to moles:

Given mass of carbon (graphite) = 0.30 g

Molar mass of carbon (graphite) = 12.01 g/mol

Number of moles of carbon (graphite) = (Given mass of carbon (graphite) / Molar mass of carbon (graphite))

Step 2: Determine the molar ratio:

From the balanced chemical equation, we can see that the molar ratio between carbon (graphite) and carbon dioxide (CO2) is 1:1.

Step 3: Calculate moles of carbon dioxide (CO2) produced:

Number of moles of carbon dioxide (CO2) = Number of moles of carbon (graphite)

Step 4: Calculate the released heat:

Released heat = (Number of moles of carbon dioxide (CO2) * Enthalpy change (∆H))

Now, let's calculate the released heat:

Number of moles of carbon (graphite) = (0.30 g / 12.01 g/mol) = 0.02498 mol

Number of moles of carbon dioxide (CO2) = 0.02498 mol

Released heat = (0.02498 mol * -11020 kJ/mol)

Therefore, the released heat from burning 0.30 g of carbon (graphite) is approximately -275.55 kJ/mol.

Learn more about Molar mass here:

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