A) Generate a graph of ln Ksp vs 1/T (K) and find the best-fitting line.  This line equation will give you the slope, which is -∆H˚/R and an intercept of ∆S˚/R. B) Determine ∆G˚ at 298K Borax is also useful as a water softener.  Hard water is caused primarily by the presence of magnesium and calcium ions, which enter the water supply from minerals (calcite, gypsum and dolomite) within an aquifer.  Hard water will form deposits that clog drains.  Borax will react with these ions in a single replacement reaction releasing free sodium ions, which do not react with water and produce deposits.   C: Write a balanced chemical equation for the reaction of Borax with calcium and magnesium ions to produce an insoluble product that will in effect, remove these ions from the water supply, thereby 'softening' the water. Please help with parts A B and C

Q: Determine the equilibrium constant for a reaction at 230.0 K if ∆G° =-13.70 kJ/mol. (R = 8.314 J/mol…

A: The relation between standard Gibbs free energy change(ΔG°) and equilibrium constant(Keq) is given…

Q: What is K for a reaction if ∆G° =-269.9 kJ/mol at 25°C? (R = 8.314 J/mol ･ K)

A: Answer :-  K = 2.0 × 1047 the equilibrium constant, K for the reaction = 2.0 × 1047…

Q: QUESTION 7: The molar volume of a certain solid is 147.0 cm³ mol-¹ at 1.00 atm and 427. 15 K, its…

A: To calculate the enthalpy and entropy of fusion of a solid given that the melting point of the solid…

Q: Determine ∆G° for a reaction when ∆G = -126.1 kJ/mol and Q = 0.043 at 298 K. (R = 8.314 J/mol ･ K)

A:

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 4.0 at 295 K? (R = 8.314 J/mol ･ K)

A: The given problem can be solved by using the formula given below as; ∆G = ∆G° + 2.303 RT log Q…

Q: 2. Using the value of standard Gibbs free energy change, AG°xn, predict the spontaneity of the…

A: The reaction is given as follows: 3NO2(g)+H2O(l)-------->2HNO3(l)+NO(g)

Q: Determine ∆G° for a reaction when ∆G = -88.9 kJ/mol and Q = 0.043 at 298 K. (R = 8.314 J/mol ･ K)

A: The objective of this question is to calculate the standard Gibbs free energy change (∆G°) for a…

Q: The ∆G° of vaporization for butane at 298 K and 1.00 atm is -2.125 kJ/mol. Calculate the pressure of…

A: The equilibrium is Butane(l)↔Butane(g)

Q: The ∆G° of vaporization for benzene at 298 K and 1.00 atm is 4.883 kJ/mol. Calculate the pressure,…

A:

Q: The discovery of the Haber process for the production of ammonia from nitrogen was a turning point…

A: First, we need to calculate the standard Gibbs free energy change (∆G°) for the reaction. The ∆G°…

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 3.0 at 295 K? (R = 8.314 J/mol ･ K)

A: The spontaneity and feasibility of reaction can be predicted by the Gibb’s free energy of that…

Q: Determine ∆G° for a reaction when ∆G = -131.1 kJ/mol and Q = 35 at 325 K. (R = 8.314 J/mol ･ K)

A:

Q: Determine ∆G° for a reaction when ∆G = -163.8 kJ/mol and Q = 0.043 at 298 K. (R = 8.314 J/mol ･ K)

A: The standard Gibb's free energy change and reaction quotient have the following relationship. ΔG =…

Q: Find Kp°  and ∆G°  for O2 (g) ↔ 2O (g), assume ideal gases If 0.150 mol of O2 (g) is placed in an…

A:

Q: Discuss the factors affecting the sign of AG in the relationship AG= AH - TAS. Give examples for…

A: Negative free energy change accompanies spontaneity of the reaction or process.

Q: Determine K for a reaction at 200 K if ∆G° =22.7 kJ/mol. (R = 8.314 J/mol ･ K)

A: Interpretation: The value of K for a reaction at 200 K is to be determined.

Q: For a reaction, ∆Ho = 363.0 kJ mol-1 and ∆So = 311.2 J K-1mol-1. Calculate the value of ∆Go  kJ…

A: Given,   ∆Ho = 363.0 kJ mol-1 .                           ∆So = 311.2 J K-1mol-1.…

Q: What is K for a reaction if ∆G° =-232.9 kJ/mol at 25°C (or 298 K)? (R = 8.314 J/mol ･ K)

A: We know that  ∆G° = - RT lnK

Q: What is K for a reaction if ∆G° =-292.8 kJ/mol at 25°C? (R = 8.314 J/mol ･ K)

A: Interpretation: The value of K for a reaction, if ∆G° = -292.8 kJ/mol at 25°C is to be determined.

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 0.14 at 295 K? (R = 8.314 J/mol ･ K)

A: Given: ∆G° = -4.5 kJ/mol Q = 0.14 Temperature = 295 K R = 8.314 J/mol ･ K

Q: Calculate the value of ArH. for the reaction below at 298 K and at 550 K. Use the data in the table…

A:

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 0.54 at 295 K? (R = 8.314 J/mol ･ K)

A:

Q: Determine ∆G° for a reaction when ∆G = -195.8 kJ/mol and Q = 35 at 325 K. (R = 8.314 J/mol ･ K)

A: Thermodynamics is branch of chemistry in which we deal with amount of heat evolved or absorbed by…

Q: Determine K for a reaction at 200 K if ∆G° =12.5 kJ/mol. (R = 8.314 J/mol ･ K)

A: Given data, T = 200 K R = 8.314 J/mol.K ∆G° =12.5 kJ/mol = 12.5 × 103 J By using the following…

Q: The discovery of the Haber process for the production of ammonia from nitrogen was a turning point…

A: Approach to solving the question: Detailed explanation: Examples: Key references:

Q: What is K for a reaction if ∆G° =-254.1 kJ/mol at 25°C? (R = 8.314 J/mol ･ K)

A: The most usual method to state about reaction's spontaneity is comparing its Gibbs energy or its…

Q: emental carbon usually exists in one of two forms: graphite or diamond. It is generally believed et…

A: In this question, we want to determine the ∆G° for this given transformation.  You can see details…

Q: Calculate Kp for the following equation with a ΔGo for C2H4O = -13.1 kJ/mole at 25.0 oC. 2C2H4(g) +…

A: The Gibbs free energy of a reaction is defined as the energy associated with a chemical reaction…

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 2.5 at 295 K? (R = 8.314 J/mol ･ K)

A: According to thermodynamics equation, dG = dG° + RTlnQ On solving above equation we get,

Q: Determine K for a reaction at 200 K if ∆G° =16.7 kJ/mol. (R = 8.314 J/mol ･ K)

A:

Q: What is K for a reaction if ∆G° =-180.3 kJ/mol at 25°C (or 298 K)? (R = 8.314 J/mol ･ K)

A:

Q: 20. What is A,G° (in kJ) at 500.0 K for the following reaction: Zn(s) + H2O(g) - ZnO(s) + H2(g)? 200…

A:

Q: Determine the equilibrium constant for a reaction at 200.0 K if ∆G° =-11.70 kJ/mol. (R = 8.314 J/mol…

A:

Q: 15) Calculate the AG°₁ AHᵒf (kJ/mol) S°(J/mol K A) +50.8 kJ rxn at 298 K using the following…

A:

Q: 2 C5H10 (1)+15 O₂ (g) → 10 CO₂ (g) + 10 H₂O(l) a. Calculate 4H of the reaction. b. Calculate 4S of…

A: Dear student ,   since you have posted multiple parts questions we will allow to solve only first…

Q: When the reaction FeO (s) + CO (g) ↔ Fe (s) + CO2 (g) takes place at 600 K, it is observed that XCO…

A: a). = equilibrium constant at 600°C =  0.900 b). where, R = Gas constant = T = temperature = =…

Q: Determine AG° for 2 NO2(g) → N2O«(g) at 25°C. Substance AGʻ† (kJ/mol) NO2 (g) 51.3 N204 (g) 97.8

A: Determine ∆G° for the given reaction ---

Q: 1 Consider the following reaction: Cu2S(s) + 02(g) = 2Cu(s) + SO2(g) Determine the estimated value…

A: Recall the given reaction Cu2Ss + O2g ⇔ 2Cus + SO2g Recall the following relations…

Q: Determine ∆G° for a reaction when ∆G = -152.3 kJ/mol and Q = 0.043 at 298 K. (R = 8.314 J/mol ･ K)…

A: We have to find value of ∆G°

Q: Determine the standard free energy change at 25 °C for the reaction 2 H2(g) + O2(g) ---> 2 H2O(g)…

A: The standard thermodynamic data for the given reactants and products at given temperature is,

Q: Calculate the AG for the vaporisation of mercury at 24°C using AH = 61.0 kJ mol-1 and AS = 89.0 J…

A:

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 1.6 at 295 K? (R = 8.314 J/mol ･ K)

A: Given: Standard Gibbs free energy change, ∆G° = -4.5 kJ/mol Reaction quotient, Q = 1.6 Temperature,…

Q: What is ∆G for a reaction where ∆G° = -4.5 kJ/mol and Q = 2.0 at 295 K? (R = 8.314 J/mol ･ K)

A:

Q: Use the ∆G = ∆H – T∆S relationship to justify why the solubility of KOH(s) in water decreases as…

A: Since S0 value for KOH(s) is greater than that for KOH(aq) Hence we can say that in dissolution of…

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.