Nitromethane (CH 3 NO 2 ) burns in air to produce significant amounts of heat. 2 CH 3 NO 2 (l) + 3/2 O 2 (g) → 2 CO 2 (g) + 3 H 2 O(l) + N 2 (g) ΔH° rxn = –1418 kJ How much heat is produced by the complete reaction of 5.56 kg of nitromethane?

Hey everyone. Our question here is asking us to calculate the heat generated by the complete combustion of 6.32 kg of nitro Benzene for this question. We're going to go ahead and use our dimensional analysis and convert from kilograms of nitrobenzene into grams into moles of nitrobenzene and then finally into killing jewels of nitrobenzene. Starting off with 6.32 kg of Nitro Benzene, We can go ahead and convert this into Graham, since we know that one kg contains 10 to the 3rd g. And to convert from grams into moles, we can go ahead and use our molar mass of nitro Benzene, Which is 123.12 g per one mole and to convert from moles into killer jewels, we can go ahead and use our standard entropy of our reaction, which is 12352 kg jewels. And this is going to be perform away of Nitro Benzene. Since we have that coefficient of four prior to nitro Benzene in our balanced chemical reaction. And the reason why we got rid of our negative sign is because we're calculating the heat generated by our combustion. So when we calculate this out and cancel out our units, We're going to end up with a total of 1.5, 9 Times 10 to the 5th killer jewels. And this is going to be our final answer. So I hope this made sense. And let us know if you have any questions

Ch.6 - Thermochemistry

All textbooks

Tro 4th Edition

Ch.6 - Thermochemistry

Problem 61

Chapter 6, Problem 61

Nitromethane (CH₃NO₂) burns in air to produce significant amounts of heat. 2 CH₃NO₂(l) + 3/2 O₂(g) → 2 CO₂(g) + 3 H₂O(l) + N₂(g) ΔH°_rxn = –1418 kJ How much heat is produced by the complete reaction of 5.56 kg of nitromethane?

Verified step by step guidance

Convert the mass of nitromethane (5.56 kg) to grams by multiplying by 1000.

Calculate the number of moles of nitromethane using its molar mass (CH3NO2). The molar mass is the sum of the atomic masses of all atoms in the molecule.

Use the stoichiometry of the balanced chemical equation to determine the relationship between moles of nitromethane and the enthalpy change (ΔH°rxn).

Calculate the total heat produced by multiplying the number of moles of nitromethane by the enthalpy change per mole of reaction (ΔH°rxn).

Ensure the units are consistent and convert the final answer to kilojoules if necessary.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the proportions of substances involved in a reaction, which is essential for calculating how much heat is produced when a specific amount of a reactant, like nitromethane, is consumed.

Enthalpy Change (ΔH)

Enthalpy change (ΔH) represents the heat absorbed or released during a chemical reaction at constant pressure. In this case, the negative value of ΔH indicates that the reaction is exothermic, meaning it releases heat. Understanding ΔH is crucial for calculating the total heat produced from the combustion of nitromethane.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To find out how much heat is produced from a given mass of nitromethane, we first need to convert the mass of nitromethane (5.56 kg) into moles using its molar mass, which is essential for applying stoichiometry in the heat calculation.

Recommended video:

Guided course

02:11

Molar Mass Concept

Related Practice

Textbook Question

Determine whether each process is exothermic or endothermic and indicate the sign of ΔH. a. dry ice evaporating b. a sparkler burning c. the reaction that occurs in a chemical cold pack used to ice athletic injuries

Textbook Question

What mass of natural gas (CH₄) must burn to emit 267 kJ of heat? CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) ΔH°_rxn = –802.3 kJ

Textbook Question

Titanium reacts with iodine to form titanium(III) iodide, emitting heat. 2 Ti(s) + 3 I₂(g) → 2 TiI₃(s) ΔH°_rxn = –839 kJ Determine the mass of titanium that react if 1.55×10³ kJ of heat is emitted by the reaction.

Textbook Question

The propane fuel (C₃H₈) used in gas barbeques burns according to the thermochemical equation: C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g) ΔH°_rxn = –2044 kJ If a pork roast must absorb 1.6×10³ kJ to fully cook, and if only 10% of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO₂ is emitted into the atmosphere during the grilling of the pork roast?

views

Textbook Question

Charcoal is primarily carbon. Determine the mass of CO₂ produced by burning enough carbon (in the form of charcoal) to produce 5.00×10² kJ of heat. C(s) + O₂(g) → CO₂(g) ΔH°_rxn = –393.5 kJ

views

Nitromethane (CH3NO2) burns in air to produce significant amounts of heat. 2 CH3NO2(l) + 3/2 O2(g) → 2 CO2(g) + 3 H2O(l) + N2(g) ΔH°rxn = –1418 kJ How much heat is produced by the complete reaction of 5.56 kg of nitromethane?

Verified video answer for a similar problem:

Key Concepts

Stoichiometry

Enthalpy Change (ΔH)

Molar Mass

Nitromethane (CH₃NO₂) burns in air to produce significant amounts of heat. 2 CH₃NO₂(l) + 3/2 O₂(g) → 2 CO₂(g) + 3 H₂O(l) + N₂(g) ΔH°_rxn = –1418 kJ How much heat is produced by the complete reaction of 5.56 kg of nitromethane?