Chapter 06: Chemical Energetics
Interactive MCQs & Virtual Chemistry Lab
Multiple Choice Questions
Q.1
Which of the following represents standard heat of formation of C2H4? →C,H4(8)
Born-Haber Cycle
Q.2
Which of the following equations , of correctly defines lattice energy MgCl2?
Q.3
Suppose there are 100 molecules of a gas initially in jar A, which is connected to an evacuated jar B. When the stopcock is opened, the positive ways of arrangement of molecules will be:
Entropy
Q.4
For a reaction to occur spontaneously,
Q.5
The calorie content of food, often expressed in Calories (keal), is fundamentally related to which thermodynamic quantity during its metabolism or combustion?
Hess's Law
Q.6
Which of the following quantities is NOT typically determined using Hess's Law?
Enthalpy Change
Q.7
Which of the following factors would lead to a greater enthalpy change of hydration (more exothermic)?
Q.9
Which of the following reactions has an enthalpy change that is equal to the standard enthalpy of formation of water, AH® 1(1,0) ?
Q.10 The enthalpy change for a reaction depends on:
Thermochemistry
Q.11
Which of the following processes would an increase in typically result in entropy of the system?
Q.12
Consider a reaction with ДH>0 and AS<0. This reaction will be:
Q.13
Which of the following is always negative in an exothermic reaction?
Q.14
The enthalpy changes when one mole of a substance burns completely in oxygen is called:
Q.15 AH for an endothermic reaction is:
Q.16 The SI unit of enthalpy is:
Q.17
Which law states that enthalpy change is independent of the path taken?
Q.18 The system that exchanges heat but not mass:
Q.19 When a bond is formed:
Q.20 The sign of AH during melting is:
Q.21
Enthalpy change of a process is measured under:
Q.22 An endothermic reaction is spontaneous when:
Q.23 The change in internal energy is zero in:
Q.24
Enthalpy of neutralization of strong acid and strong base is approximately:
Q.25
The standard enthalpy of formation of elements in their standard state is:
Q.26
Which of the following is a state function?
Q.27 Standard conditions include except:
Q.28
The enthalpy atomization of an element is always:
Q.29 The enthalpy of solution is:
Q.30 A reaction is spontaneous when:
Q.31 If a chemical reaction has AH =-100 kJ/mol, it is:
Q.32 The enthalpy of sublimation involves:
Q.33
The enthalpy change when one mole of ionic compound is dissolved in water is:
Q.34
Which of the following is an extensive property?
Q.35 Enthalpy of fusion is the heat required to:
Q.36
Which reaction releases more energy?
Q.37 AHf° of Hag) is:
Q.38 Standard enthalpy change refers to:
Q.39
Which gas has highest molar enthalpy of combustion?
Q.40 Energy stored in chemical bonds is:
Q.41
Which of the following affects bond energy? Bond
Q.42
Which of the following has the highest bond energy?
Q.43
The energy required to break a chemical bond is called:
Q.44 The equation q = meAT is used to find:
Q.45
Which of the following is used to measure heat changes?
Q.46
Which following maximum heat capacity?
Q.47
Specific heat capacity is amount of heat needed to raise temp of:
Q.48 Heat of combustion of H2 is used to determine:
Q.49 AH = q at constant:
Q.50 Enthalpy change in hydration depends on:
Q.51
In an exothermic reaction, the energy of products is:
Q.52
The term "lattice energy" is applicable to:
Q.53 A negative lattice energy implies:
Q.54
Which factor affects lattice energy?
Q.55 The unit of lattice energy is:
Q.56 Born-Haber cycle is used to calculate:
Q.57
Which step in the Born-Haber cycle is always endothermic?
Q.58
What type of reaction has a negative AH and AS?
Q.59
Which of the following causes entropy to increase?
Q.60 AH is negative and AS is positive. Then reaction is:
Q.61
A process with increase in entropy 63. Which is not a path function? and enthalpy is spontaneous at:
Q.62 An increase in entropy favors:
Q.64 AG = 0 indicates:
Q.65 A reaction is feasible it:
Reaction Energy Profile Lab
Drag the sliders to see how reactant, transition, and product energy affects activation energy.
Activation Energy (Ea): 70 kJ/mol
Enthalpy Change (dH): -40 kJ/mol