29 Questions
Which equation represents the behavior of an ideal gas?
PV = nRT
What is the value of the gas constant R in units of L atm K-1 mol-1?
0.082
Which type of variables are independent of the size of the system?
Intensive variables
What kind of gas does not obey the PV = nRT equation?
Real gas
If a variable x is a state function, what remains the same when going from State I to State II?
$\Delta x(a)$
For any cyclic process, what is the value of $\Delta x$?
$0$
Which region is characterized by properties such as Temperature, Pressure, and Volume?
System
In which type of system can both energy and matter be exchanged between the system and its surroundings?
Open system
What is the region outside the system and separated from the system by a boundary called?
Surroundings
Which type of system allows only energy transfer, either as work or by heat transfer?
Isolated system
Which type of system does not allow for the exchange of energy or matter?
Isolated system
What is the term used for the organized form of energy transfer in thermodynamics?
Work
Which method involves a 2-step reaction for the formation of CO2?
Method 2
What is the standard enthalpy of formation of H2O (l) at 298 K?
-285.83 kJ mol-1
What is the reference state of an element in standard enthalpies of formation?
Its most stable state at specified temperature and pressure
What does Hess's law state about the enthalpy of formation of compounds?
It is additive and independent of the reaction path
Which law is used to calculate the enthalpy change when substances are formed from their elements?
Hess's Law
What is the relationship between enthalpy change (∆H) and internal energy change (∆U) in a chemical reaction according to the First Law of Thermodynamics?
∆H is always less than ∆U
What does the equation qP = qV + RT(∆n) represent in the context of gas phase reactions?
The enthalpy change due to a change in the number of moles of gas reactants
What is the purpose of a constant-volume bomb calorimeter in thermodynamic experiments?
To ensure no heat enters or leaves the system during a reaction
What does the equation qcal =Ccal ∆t represent in the context of calorimetry?
The heat exchange during the reaction in a bomb calorimeter
In a constant-pressure bomb calorimeter, what principle is used to relate the heat changes of the compound and water?
The law of conservation of energy
For a combustion reaction in a constant-volume calorimeter, if q = 1364.34 kJ mol-1 at 298 K, what is the value being measured?
Enthalpy change of combustion
What is the relationship between enthalpy change (∆H) and internal energy change (∆U) according to Hess's Law?
They are independent
In a chemical reaction, if the enthalpy changes for the individual steps are known, what can be said about the overall enthalpy change according to Hess's Law?
It is equal to the sum of enthalpy changes for individual steps
If a reaction takes place in a series of steps, what does the stoichiometric coefficients of product and reactant represent?
The smallest integers consistent with the reaction
What role do enthalpy and internal energy play in chemical reactions according to the First Law of Thermodynamics?
They provide information about heat changes in reactions
If a reaction has ∆n = -1, what can be concluded about the enthalpy change (∆H) based on the formula ∆H = ∆U + RT(∆n)?
∆H is negative
Why is it important to consider enthalpy changes in chemical reactions?
To predict if a reaction is exothermic or endothermic
Explore the concept of the First Law of Thermodynamics in chemical reactions, focusing on enthalpy changes and how they are related to internal energy and pressure-volume work. Learn about the significance of physical states (gas, liquid, solid) and temperature in determining reaction enthalpy.
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