Nitromethane (CH3NO2) burns in air to produce significant amounts of heat via the following reaction:
2CH3NO2(l)+32O2(g)→2CO2(g)+3H2O(l)+N2(g)ΔH∘rxn=−1418kJ
Part A
How much heat is produced by the complete reaction of 4.93 kg of nitromethane?
Express your answer to three significant figures and include the approp
Well, well, well, looks like we have a burning question here!
To find out how much heat is produced, we need to use the good old mole-to-mole ratio. So let's get started, shall we?
First, we need to convert the mass of nitromethane (4.93 kg) into moles. The molar mass of nitromethane (CH3NO2) is approximately 61.04 g/mol.
4.93 kg x (1000 g/1 kg) x (1 mol/61.04 g) = approximately 80.7 mol
Now that we have the moles of nitromethane, we can use the stoichiometry of the reaction to find the heat produced. According to the balanced equation provided, it takes 2 moles of nitromethane to produce -1418 kJ of heat.
So let's do some math, my friend:
80.7 mol x (-1418 kJ/2 mol) = approximately -57,000 kJ
Voila! The heat produced by the complete reaction of 4.93 kg of nitromethane is approximately -57,000 kJ.
Remember, negative heat values mean that heat is being released (exothermic reaction), so it's gonna get hot in here!
To find the amount of heat produced by the complete reaction of 4.93 kg of nitromethane, we will use the given molar mass of nitromethane (61.04 g/mol) and the given molar enthalpy of reaction (-1418 kJ/2 mol).
First, convert the mass of nitromethane to moles:
Mass = 4.93 kg = 4930 g
Moles of CH3NO2 = (4930 g) / (61.04 g/mol) = 80.71 mol
Next, use the stoichiometric coefficients from the balanced equation to determine the mol-to-mol ratio between CH3NO2 and heat released:
2 mol of CH3NO2 produce -1418 kJ of heat
Now, calculate the heat produced by converting the moles of nitromethane to heat:
Heat = (80.71 mol CH3NO2) × (-1418 kJ/2 mol CH3NO2)
Heat = -57479.88 kJ
Finally, round the answer to three significant figures due to the given value:
Heat ≈ -57480 kJ
Therefore, the amount of heat produced by the complete reaction of 4.93 kg of nitromethane is approximately -57480 kJ.
To calculate the amount of heat produced by the complete reaction of 4.93 kg of nitromethane, we need to use the given equation and the molar mass of nitromethane.
Step 1: Find the number of moles of nitromethane.
The molar mass of nitromethane (CH3NO2) is:
C: 1 x 12.01 g/mol = 12.01 g/mol
H: 3 x 1.01 g/mol = 3.03 g/mol
N: 1 x 14.01 g/mol = 14.01 g/mol
O: 2 x 16.00 g/mol = 32.00 g/mol
Total molar mass = 12.01 + 3.03 + 14.01 + 32.00 = 61.05 g/mol
Now, we'll convert the given mass from kg to grams:
4.93 kg × 1000 g/kg = 4930 g
Next, we'll calculate the number of moles of nitromethane:
moles = mass / molar mass
moles = 4930 g / 61.05 g/mol
moles ≈ 80.7 mol
Step 2: Calculate the heat produced.
Using the balanced equation, we know that 2 moles of nitromethane produce -1418 kJ of heat.
So, 80.7 moles of nitromethane will produce:
heat = (80.7 mol / 2 mol) x -1418 kJ
heat ≈ -57633.9 kJ
Since heat is a form of energy, it is always positive. Therefore, we need to take the absolute value of the result:
heat = |-57633.9| kJ ≈ 57634 kJ
Expressing the answer to three significant figures, the amount of heat produced by the complete reaction of 4.93 kg of nitromethane is approximately 57600 kJ.
You made a typo on the equation. It should be
2CH3NO2(l) + 3/2O2(g)→2CO2(g)+3H2O(l)+N2(g).......ΔH∘rxn=−1418kJ
1418 kJ is produced by 2*molar mass CH3NO2 or
1418 kJ is produced by 122 g so heat produced by 4.93 kg will be
1418 kJ x (4930/122) = ? kJ