Many chemical reactions proceed at rates that depend on the temperature. Discuss this from the point of view of the Boltzmann distribution.

Q: The activation energy of a certain gas reaction is 15.4 kJ/mol. Estimate the fraction of collisions…

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Q: 6. What is the difference between kinetically controlled and thermodynamically controlled processes?

A: Thermodynamics: about "if"  • tells whether a cycle or a response can happen (is there a reduction…

Q: Which of the following reaction coordinate diagrams explains the formation of different…

A: The thermodynamic product has higher activation energy is more stable whereas the kinetic product…

Q: For the reaction C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g), ΔrU⦵ = −1373 kJ mol−1 at 298 K.…

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Q: Write down the expression for the equilibrium constant of the reaction N2(g) + 3 H2(g) ~ 2 NH3(g) in…

A: The given reaction is, N2(g) + 3H2(g) ---> 2 NH3(g)

Q: If the entropy of the system increases during a reversible process, the entropy change of the…

A: The entropy change of the system depends upon the randomness. As the randomness of the system…

Q: For any reaction to occur spontaneously gibbs free energy should be negative, explain this statement…

A: Gibbs free energy:- It is the useful work obtained in a chemical reaction. It is always negative…

Q: In some reaction mechanism there is competition between enthalpy and entropy of reaction. some…

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Q: Phosphorous and chlorine gases combine to produce phoshorous trichloride delta G at 298K for this…

A: The balanced reaction taking place is  P2 + 3 Cl2 ------> 2 PCl3  Hence the reaction quotient of…

Q: Check out the change in entropy round your answer to two significant digits and be sure it has a…

A: The possible number of ways that Cl and Br atoms can be adsorbed initially is 16.Given that Br atom…

Q: Gibbs free energy change

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Q: NH3 is an important molecule for a wide range of synthetic and agricultural applications. Under…

A: 1. ∆H0 (rxn) = 46 KJ/mol; ∆S0 (rxn) = 130 JK-1mol-1  2. The reaction is endothermic. 3. The would…

Q: "At steady state, free energy is continuously put into the system. In dynamic equilibrium, net free…

A: The energy is constantly supplied to the system in order to maintain a free energy state which is…

Q: Compare the expressions for the relationship between the change in free energy of a reaction and its…

A: Given: To compare the expressions for the relationship between the change in free energy of a…

Q: For an isolated system, maximum entropy will occur at half-life critical condition equilibrium start…

A: Isolated system is a system where energy cannot cross the boundary of the system

Q: A closed system will spontaneously proceed in a direction of maximum randomness

A: Entropy is defined as a measure of disorderness or unevenness of the system

Q: Is the electronic contribution to the reaction constant in the reaction of 1 nitrogen atom with 1…

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Q: Consider the reaction: SO2(g) +1/2 O2(g) → SO3(g). If the initial pressures of both SO2 and O2 are…

A: given :-                  So2 (g) + 1/2 O2 (g) → So3 (g)  Initial pressure of So2 = 1.00 bar…

Q: Describe how ΔH-T ΔS functions as a criterion of a spontaneous reaction.

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Q: what is the name of the symbol of the single thermodynamic quantity (function) which determines…

A: what is the name of the symbol of the single thermodynamic quantity (function) which determines…

Q: Which of the following measures the molecular randomness of a reaction? a. Enthalpy O b. Entropy O…

A: Here some physical parameters are given.

Q: Relate entropy to disorder in a molecular system (energy dispersal).

A: Entropy is a thermodynamic property that helps to estimate the thermal energy per unit temperature…

Q: The urms of H2 molecules at 273K is 1.84×103m/s. At what temperature is urms for H2 1.8 times…

A: Since the urms of any molecule is given by  Hence we can say  urms T1 / urms T2 = (T1 / T2)1/2…

Q: Use the data in the table to calculate the ΔH°rxn of the following reaction at 298 K: HI(g) +…

A: Generally in the chemical reaction, the enthalpy of reaction is denoted by (ΔHrxn) is the difference…

Q: For a certain process, ∆G is large and negative. Does this mean that the process necessarily has a…

A: No. All such process in which ∆G is large and negative does not necessarily has a low activation…

Q: Enumerate atleast three examples each for a spotaneous reaction and a nonspontaneous reaction

A: Spontaneous reaction : These are the reactions which occur on their own that means no external…

Q: For a reaction 2A+B2-2AB AG= 34.8 kJ-mol-1 and AG = 42.4 kJ.mol-1 at a temperature of 143 K.…

A: Given data : 2A + B2 ---->2AB Standard Gibbs free energy = 42.4KJmol-1 Gibbs free energy =…

Q: Calculate the change in entropy. Round to three sig figs.

A: The entropy can be determined using Boltzmann equation of entropy.The 'Boltzmann' equation for…

Q: What happens to the entropy of an isolated system during an irreversible process?

A: For isolated system, there is no exchange of heat or energy between system and surrounding.  Hence,…

Q: Please repeat the last problem at P= 5 bar. a. Based on the reaction alone, would one expect the…

A: A Reaction equlibrium is changed with pressure. It changes according to La chatelier principle

Q: Explain the Gibbs-Duhem equation?

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Q: Consider the following reaction: CO2(g)+CCl4(g)⇌2COCl2(g) Calculate ΔrG for this reaction at 125…

A: Given, Consider the following reaction:CO2(g)+CCl4(g)⇌2COCl2(g) PCO2= 0.100 barPCCl4= 0.185…

Q: What is the correct Ksp expression for Lead(II) Chloride dissolving in water?

A: In general , a salt of type AxBy which dissociates as,                                AxBy ---->…

Q: Use the reaction for the formation of NH3 from its elements N2(g) and H2(g) . This reaction has the…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: For a given process at constant pressure, w is positive. This means that the process involves

A: In chemical thermodynamics, work done is calculated as: w = -p(V2-V1)   Given, work done is positive…

Q: Consider the reaction 2 NO21g2 ¡ N2O41g2. Calculate ∆G at 298 K if the partial pressures of NO2 and…

A: Given: Partial pressure of NO2 = 0.40 atm Partial pressure of N2O4 = 1.60 atm Temperature (T) = 298…

Q: Determine the ΔS system given the reaction :         C6H12O6 (s) + O2(g) --------------→ CO2 (g) +…

A: The give reaction is   C6H12O6 (s) + O2(g) → CO2 (g) + H2O (l)  the change in entropy, ΔS system  of…

Q: - What is a catalyst? - Draw a potential diagram explaining the function of a catalyst and compare…

A: Definition of catalyst: A catalyst is a synthetic substance that influences the rate of a chemical…

Q: In some reaction mechanism there is competition between enthalpy and entropy of reaction.some…

A: Entropy is a measure of the randomness in the thermodynamic system. More the randomness in the…

Q: State and explain Le Chatelier 's principle in terms of thermodynamic quantities. Could there be…

A: Le Chatelier 's principle states that if a system in equilibrium is subjected to a change in…

Q: se the Maxwell-Boltzmann distribution curve to explain why adding a catalyst will speed up the rate…

A: Adding catalyst increases the number of particles that have greater energy than the activation…

Q: Check out the change in entropy round your answer to two significant digits and be sure it has a…

A: The new number of microstates of chlorine = 16The original number of microstates when Cl and Br…

Q: For the reaction 2C6H$COOH(s) + 13 O2(g) → 12CO2(g)+6 H2O(g), A,U© = -772.7 kJ mol·' at 298 K.…

A: Consider the following reaction: 2C6H5COOH(s) + 13O2(g) → 12CO2(g) + 6H2O(g) ∆rU°=-772.7…