Calculate the energy required to produce 7.00 mol ClO on the basis of the following balanced equation.
2Cl(g) + 7O(g) + 130 kcal 2ClO(g)

Question

Calculate the energy required to produce 7.00 mol ClO on the basis of the following balanced equation.
2Cl(g) + 7O(g) + 130 kcal  2ClO(g)

BlackTom AI · Accepted Answer

Restating the problem in my own words: We are given a balanced reaction where producing 2 ClO molecules requires 130 kcal of energy. The task is to find the energy needed to produce 7.00 mol of ClO.
Option A: 7.00 kcal. This would imply an energy per mole that is far smaller than the given energy per 2 moles. Since the reaction energy is tied to producing ClO, this value does not align with the stoichiometry or the provided 130 kcal for 2 moles, so it is incorrect.
Option B: 65 kcal. This is exactly half of 130 kcal, which might tempt someone to divide by 2, perhaps thinking in terms of per-mole energy. However, the 130 kcal corresponds to the production of 2 moles of ClO, not 1 mole. Therefore halving it would only be appropriate if we produced 1 mole of ClO, not 7 moles, making this option inaccurate for the given quantity.
Option C: 130 kcal. This value represents the energy for producing 2 moles of ClO, not the 7.00 moles specified. If we produced 2 moles, 130 kcal would be correct, but for 7.00 moles, the energy required would scale with the amount of product, so this option underestimates the needed energy.
Option D: 455 kcal. This matches the proper scaling: the reaction energy is 130 kcal per 2 moles of ClO. First find the factor: 7.00 mol ClO ÷ 2 mol = 3.5. Then multiply 130 kcal by 3.5 to get 455 kcal. This correctly accounts for the stoichiometry and the amount of product requested.
In summary, the key is recognizing the 130 kcal corresponds to producing 2 mol of ClO, and then scaling by 7.00/2 = 3.5, yielding 130 × 3.5 = 455 kcal. The other options fail because they either ignore the per-2-moles energy, misapply scaling, or attempt to apply energy per mole incorrectly.

Chemistry (H) - Varnold - Preparatory Academy - 2nd Semester - 2024/2025 2025 Thermochemistry Practice Test

Calculate the energy required to produce 7.00 mol ClO on the basis of the following balanced equation. 2Cl(g) + 7O(g) + 130 kcal 2ClO(g)

查看解析

登录即可查看完整答案

类似问题

The heat of combustion of ethane, C2H6, is 1560 kJ/mol. What is the heat of combustion of ethane, in kJ per gram?

Consider the equilibrium dissociation of N2O4(g) to NO2(g). N2O4(g) ⇌ 2NO2(g) Using your knowledge of Lewis structures and bond energies (bond breaking vs. bond forming) to predict whether this reaction is

Calculate H for the reaction of sulfur dioxide with oxygen. 2SO(g) + O(g) 2SO(g) (HSO(g) = –296.8 kJ/mol; HSO(g) = –395.7 kJ/mol)

The amount of heat released by the complete burning of 1 mole of a substance is its ____.

One mole of hydrogen is burned in oxygen to produce water in the gas phase, H = 285.8 kJ. What is the energy change when 1 mole of water, in the gas phase, decomposes to form hydrogen and oxygen?

更多留学生实用工具

考试浏览器助手

风格化写作助手

论文查重助手

文献引用助手

课堂转译助手

课堂笔记助手

Quiz搜索助手

学校历年真题

智能刷题助手

智能匹配练习

希望你的学习变得更简单