Textbook Question
Write balanced equations for the formation of the following compounds from their elements. (b) Sucrose (table sugar, C12H22O11)
622
views
Ch.9 - Thermochemistry: Chemical Energy
Chapter 9, Problem 103c
Write balanced equations for the formation of the following compounds from their elements. (c) Dichloromethane (a liquid, CH2Cl2)
Verified Solution
Video duration:
1m
This video solution was recommended by our tutors as helpful for the problem above.Was this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Balanced Chemical Equations
A balanced chemical equation represents a chemical reaction where the number of atoms for each element is the same on both sides of the equation. This is crucial for obeying the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Balancing involves adjusting coefficients in front of compounds to ensure that the total number of each type of atom is equal.
Recommended video:
Guided course
01:32
Balancing Chemical Equations
Formation Reactions
A formation reaction is a specific type of chemical reaction where a compound is formed from its constituent elements in their standard states. For example, when forming dichloromethane (CH2Cl2), chlorine gas (Cl2) and carbon (C) in its solid form, along with hydrogen gas (H2), are combined. Understanding formation reactions is essential for writing accurate equations for compound synthesis.
Recommended video:
Guided course
02:34Enthalpy of Formation
Standard States of Elements
The standard state of an element refers to its physical state and form at a specified temperature and pressure, typically 25°C and 1 atm. For example, carbon is solid (graphite), hydrogen is a gas (H2), and chlorine is also a gas (Cl2) at these conditions. Recognizing the standard states of elements is vital for correctly writing formation reactions and ensuring that the reactants are represented accurately.
Recommended video:
Guided course
03:55Element States of Matter
Related Practice
Textbook Question
Write balanced equations for the formation of the following compounds from their elements. (a) Ethanol (C2H6O)
378
views
Textbook Question
Write balanced equations for the formation of the following compounds from their elements. (b) Sodium sulfate
340
views
Textbook Question
Sulfuric acid (H2SO4), the most widely produced chemical in the world, is amde yb a two-step oxidaiton of sulfur to sulfur trioxide, SO3, followed by reaciton with water. Calculate ΔH°f for SO3 in kJ/mol, given the following data: S(s) + O2(g) → SO2(g) ΔH° = -296.8 kJ SO2(g) + 1/2 O2(g) → SO3(g) ΔH° = -98.9 kJ
1123
views
Textbook Question
Calculate ∆H°f in kJ/mol for benzene, C6H6, from the following data: 2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(l) ∆H°=-6534 kJ ∆H°f (CO2) = -393.5 kJ/mol ∆H°f(H2O) = -285.8 kJ/mol
3468
views
1
rank
Textbook Question
The standard enthalpy change for the reaciton of SO3(g) with H2O(l) to yield H2SO4(aq) is ΔH° = -227.8 kJ. Use the information in Problem 9.104 to calculate ΔH°f for H2SO4(aq) in kJ/mol. [For H2O(l), ΔH°f = -285.88 kJ/mol.]
3136
views