Consider the gas-phase reaction 2 ammonia (g) + 2 oxygen (g) 1 dinitrogen monoxide (g) + 3 water (g) Calculate the difference in chemical potential of dinitrogen monoxide (g) at a partial pressure of 0.902 atm from the standard state chemical potential. That is, what is the value of μ0.902 - μº? You may assume that the gasses behave ideally and the reaction occurs at standard temperature. kJ/mol

Consider the gas-phase reaction 2 ammonia (g) + 2 oxygen (g) 1 dinitrogen monoxide (g) + 3 water (g) Calculate the difference in chemical potential of dinitrogen monoxide (g) at a partial pressure of 0.902 atm from the standard state chemical potential. That is, what is the value of μ0.902 - μº? You may assume that the gasses behave ideally and the reaction occurs at standard temperature. kJ/mol

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 91QRT: Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium...

See similar textbooks

Similar questions

Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
Use the following data to calculate the enthalpy of solution of sodium perchlorate, NaClO4: fH(s)=382.9kJ/mol and fH(aq,1m)=369.5kJ/mol
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70C
6. When the ideal-gas reaction A+B=C+Dhas reached equilibrium, state whether or not each of the following relations must be true. Here n¡ is the number of moles of species i in equilibrium, P, is the partial pressure of i, and µ; is the chemical potential of i. Here a simple True or False answer is sufficient. (a) nc+np=nA +ng (b) Pc+Pp=PA+PB (c) na=ng (d) nc=na (e) If only A and B are present initially, then nc=np (f) Ha + HB= Hc+ Hp no matter what the initial composition. (g) If only A and B are present initially, then in equilibrium we must have nc # 0. (h) The equilibrium constant Kp(T)= PĄPB/(PcPp). (i) The value of –RT In Kp(T) = µE(T)+µ8(T)– H3(T) –- H§(T). ) The equilibrium constant is independent of the total pressure.
Camphor 1C10H16O2 melts at 179.8 °C, and it has a particularly large freezing-point-depression constant, Kf = 40.0 °C>m. When 0.186 g of an organic substance of unknown molar mass is dissolved in 22.01 g of liquid camphor, the freezing point of the mixture is found to be 176.7 °C. What is the molar mass of the solute?
C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.d) Explain the effect on equilibrium of:i) Increasing temperatureii) Increasing pressureiii) Decreasing the concentration of oxygeniv) Increasing the concentration of carbon dioxidev) Adding a catalyst
Camphor (C10H16O) melts at 179.8 °C, and it has aparticularly large freezing-point-depression constant,Kf = 40.0 °C/m. When 0.186 g of an organic substance of unknownmolar mass is dissolved in 22.01 g of liquid camphor,the freezing point of the mixture is found to be 176.7 °C.What is the molar mass of the solute?
7. The solubility, C, of sucrose in water, expressed as grams of sucrose per 100 g of solvent, is given as below t/°C C/g 0 179.2 10 20 203.9 190.5 30 219.5 [ΔΗ (a) Draw an appropriate graph to determine the molar enthalpy of solution of sucrose in the temperature range 0 to 40°C. (b) 50mL of saturated solution of benzoic acid at 25°C requires 12.8 mL of 0.05 M NaOH to completely neutralize. What is the solubility of benzoic acid in g/L water at 25°C. so ln,m 40 238.1 = 4.96 kJ/mol, Cbenzoic acid = 1.56g/L]
Calculate the Gibbs free energy of the reaction from mixing 50 mL each of 0.50 M AgNO3(aq) solution and 1 M of NaCl(aq) to form AgCl(s) at 25°. The Ksp of AgCl is 6.0 × 10—11 at 25 °C.
The sealed containers of fizzy drinks contain dissolved CO2. This dissolved CO2 is in equilibrium with a small quantity of gaseous CO2 at the top of the container. (a) The partial pressure of CO2 gas in a 250 cm3 can of fizzy drink is 3.0 atm at 25 0C. What is the concentration of CO2 in the fizzy drink? (b) If the can contain only the mass of CO2 1.09g as a gas, calculate the pressure in the can when it is stored at 25 0C. (c) The maximum pressure that a can of fizzy drink can withstand is 7 atm. Using the graph below, determine the maximum temperature at which a can, can be stored safely. (concentration=0.093M
In a constant‑pressure calorimeter, 65.0 mL65.0 mL of 0.350 M Ba(OH)20.350 M Ba(OH)2 was added to 65.0 mL65.0 mL of 0.700 M HCl.0.700 M HCl. The reaction caused the temperature of the solution to rising from 23.61 ∘C23.61 ∘C to 28.38 ∘C.28.38 ∘C. If the solution has the same density and specific heat as water (1.00 g/mL1.00 g/mL and 4.184J/g⋅°C,)4.184J/g⋅°C,) respectively), what is Δ?ΔH for this reaction (per mole H2OH2O produced)? Assume that the total volume is the sum of the individual volumes.
At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 2 B(g) = C(g) + 2 D(g) were found to be PA = 4.24 atm, PB = 5.83 atm, Pc = 4.52 atm, and Pp = 4.85 atm. %3| What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ AGXN = mol