Question

Derive the general form of the Gibbs equation and apply it to the following problem: 4...

Derive the general form of the Gibbs equation and apply it to the following problem: 4 mol of water is heated at constant pressure from 30°C to 40°C. Calculate the change in entropy when cp = 75.312 J °C-1 mol-1 .

Homework Answers

Answer #2

answered by: anonymous
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the change in entropy (in J/K) when 38.7 g of nitrogen gas is heated at...
Calculate the change in entropy (in J/K) when 38.7 g of nitrogen gas is heated at a constant pressure of 1.50 atm from 22.9 ºC to 88.2 ºC. (The molar specific heats are Cv is 20.8 J/(mol-K) and Cp is 29.1 J/(mol-K) .)
Calculate the change in entropy (in J/K) when 52.8 g of nitrogen gas is heated at...
Calculate the change in entropy (in J/K) when 52.8 g of nitrogen gas is heated at a constant pressure of 1.50 atm from 16.5 ºC to 62.8 ºC. (The molar specific heats are Cv is 20.8 J/(mol-K) and Cp is 29.1 J/(mol-K) .)
In the following problem please answer question C The temperature dependent Cp of carbon dioxide is...
In the following problem please answer question C The temperature dependent Cp of carbon dioxide is experimentally determined to be Cp = a + bT + c/T2 where a, b, and c are constants and Cp is given in units of J/mol·K a. Derive an expression for the amount of heat required to raise the temperature CO2 from T1 to T2 as a function of a, b, and c. b. Calculate the heat required to raise the temperature of 1...
This problem examines the effects of mixing water at two different temperatures and/or two different phases,...
This problem examines the effects of mixing water at two different temperatures and/or two different phases, such as dropping ice cubes into warm water. Assume that heat of fusion is 333.55 J/g, that CP for ice is constant at 2.11 J/(g·K), and CP for liquid water is constant at 4.19 J/(g·K). You can assume CP approximately equals CV for solids and liquids. For each of the following cases, assume the mixing is adiabatic and carried out at atmospheric pressure. Find...
Diamond a. At 298 K, what is the Gibbs free energy change G for the following...
Diamond a. At 298 K, what is the Gibbs free energy change G for the following reaction? Cgraphite ->  Cdiamond b. Is the diamond thermodynamically stable relative to graphite at 298 K? c. What is the change of Gibbs free energy of diamond when it is compressed isothermally from 1 atm to 1000 atm at 298 K? d. Assuming that graphite and diamond are incompressible, calculate the pressure at which the two exist in equilibrium at 298 K. e....
Carbon dioxide is an important greenhouse gas. Calculate the enthalpy change for a 66.5g sample of...
Carbon dioxide is an important greenhouse gas. Calculate the enthalpy change for a 66.5g sample of CO2 heated from 0.6 C to 50.0 C at constant pressure assuming (a) that Cp,m is not a f(T) and (b) where Cp,m is a f(T). Cp,m(CO2) = 27.11 J/molK at 25 C and a = 44.22 J/mol K, b=0.00879 J/molK^2 and c=-8.62x10^5 K/mol. How does this energy change compare to the average intermolecular force?
At 0,00℃, for H2O (l) the saturation pressure P = 4,581 dry
At 0,00℃, for H2O (l) the saturation pressure P = 4,581 dry (i.e., the water vapor equilibrium pressure) and the vaporization heat, ?vapHm = 45,067 kJ mol-1. The steam can be regarded as an ideal gas. a) Calculate water pressure at 100,00?C with the assumption that ?vapHm is a constant between 0,00 and 100,00℃. b) Between 0,00 and 100,00℃, ?Cp,m for water evaporation can be adapted to the expression ?Cp,m = (-51,22 + 0,03153T) J K-1 mol-1. Derive an expression between 0,00 and 100,00?C for ?vapHm as a function of T as well as calculate P at 100?C.
The following data are available for liquid ethanol at 20 C: M.W. = 46.07, Density =...
The following data are available for liquid ethanol at 20 C: M.W. = 46.07, Density = 0.7893 g/cc, Coefficient of thermal expansion = 1.12x10^-3 K^-1, Isothermal compressibility = 1.0x10^-4 bar^-1 (a) Estimate the difference (Cp-Cv) for liquid ethanol at 20 C in J/mol K (b) 10 liters of liquid ethanol at 20 C is compressed isothermally from initial pressure of 1 bar to a final pressure of 50 bar. For this process, calculate the enthalpy and entropy change of the...
When heated, calcium carbonate (calcite) decomposes to form calcium oxide and carbon dioxide gas CaCO3(s) <---->...
When heated, calcium carbonate (calcite) decomposes to form calcium oxide and carbon dioxide gas CaCO3(s) <----> CaO(s) + CO2(g) Using the data below, calculate the equilibrium partial pressure of CO2(g) over a mixture of solid CaO and CaCO3 at 500 ◦C if ∆CP,m for the reaction is independent of temperature over the temperature range between 25 ◦C and 500 ◦C ...............................CaO(s)..........CO2(g).............. CaCO3(s) ∆H◦ f (kJ/mol) .......−635.09 ......−393.51 ............−1206.92 S◦ m (J / mol K) ......39.75 .........213.74 .................92.90 CP,m (J /...
In this problem, 1.00 mol of an ideal diatomic gas is heated at a constant wolume...
In this problem, 1.00 mol of an ideal diatomic gas is heated at a constant wolume from 300 to 6000 K. (a) Find the increase in the internal energy of the gas, the work done by the gas, and the heat absorbed by the gas. (b) Find the same quantities if the gas is heated from 300 to 600 K at constant pressure. Use the first law of thermodynamics and your results form (a) to calculate the work done by...