I feel like this question is pretty easy, but I can't seem to figure out how to go about solving it. It's like the solution is on the tip of my tongue:

Question

I feel like this question is pretty easy, but I can't seem to figure out how to go about solving it. It's like the solution is on the tip of my tongue:

Nitromethane (CH3NO2) burns in air to produce significan amounts of heat.

2 CH3NO2(l) + 3/2 O2(g) -> 2 CO2(g) + 3 H2O(l) + N2(g)
ΔHo rxn = -1418kJ

How much heat is produced by the complete reaction of 6.90kg of nitromethane?

Answer 1

So you get 1418 kJ for every 2*61 g nitromethane. How much will you get for 6900 g.

1418 kJ x (6900/2*61) = ?

Answer 2

Just as I thought, it was much easier than I was making it out to be haha

Thank you!

Answer 3

To determine the amount of heat produced by the complete reaction of 6.90 kg of nitromethane, we can use the given enthalpy of reaction (ΔH°rxn) and the stoichiometry of the reaction.

The molar mass of nitromethane (CH3NO2) is calculated as follows:
Molar mass of C = 12.01 g/mol
Molar mass of H = 1.0079 g/mol
Molar mass of N = 14.01 g/mol
Molar mass of O = 16.00 g/mol

Thus, the molar mass of nitromethane (CH3NO2) is:
(12.01 g/mol × 1) + (1.0079 g/mol × 3) + (14.01 g/mol × 1) + (16.00 g/mol × 2) = 61.04 g/mol

Now, we need to calculate the number of moles of nitromethane:
Number of moles = Mass / Molar mass

Number of moles = 6900 g / 61.04 g/mol = 113 moles

Now that we know the number of moles of nitromethane, we can use the stoichiometric coefficients of the balanced equation to relate it to the heat produced:

From the balanced equation:
2 moles of CH3NO2 produce -1418 kJ of heat

Therefore, 113 moles of CH3NO2 will produce:
(113 moles x -1418 kJ) / 2 moles = -79927 kJ

Therefore, the complete reaction of 6.90 kg of nitromethane will produce approximately 79927 kJ of heat.

Answer 4

To calculate the amount of heat produced by the complete reaction of 6.90 kg of nitromethane, you need to use the given enthalpy change of the reaction (ΔHo rxn) and the molar mass of nitromethane.

Here's how you can solve it:

1. Determine the molar mass of nitromethane (CH3NO2).
- The molar mass of carbon (C) is 12.01 g/mol.
- The molar mass of hydrogen (H) is 1.01 g/mol.
- The molar mass of nitrogen (N) is 14.01 g/mol.
- The molar mass of oxygen (O) is 16.00 g/mol.
- Add up these atomic masses to find the molar mass of nitromethane.

2. Convert the given mass of nitromethane into moles.
- Divide the mass (6.90 kg) by the molar mass of nitromethane to get the number of moles.

3. Use the stoichiometry of the balanced equation to find the amount of heat produced.
- Based on the balanced equation, you can see that 2 moles of nitromethane produce -1418 kJ of heat.
- Use the moles of nitromethane obtained in step 2 to set up a ratio and calculate the amount of heat produced.

4. Perform the calculation.
- Multiply the number of moles obtained in step 2 by the ratio of heat produced to moles of nitromethane from step 3.

5. Round the final answer to an appropriate number of significant figures.

By following these steps, you should be able to calculate the amount of heat produced by the complete reaction of 6.90 kg of nitromethane.