Complete calculation with the detail explanation is given as below:-
1. The molar heat capacity of iridium is given by | Co,m=24.80 + 0.00597* Calculate the...
10 points. 1. The molar heat capacity of iridium is given by Cam 24.80 +0.00597"T Calculate the change in entropy if 75.0 grams of iridium is heated from O'C to 1500°C. 2. The United State
- Laticise E3B.7(a). P3B.3 The molar heat capacity of trichloromethane (chloroform, CHCI) range 240 K to 330 K is given by Cpm/(JKmol"!) = 91.47 +7.5 x 10 Calculate the change in molar entropy when CHCl, is heated from 273 K to 300 K the range 200 K to 400 K is given by
The standard molar entropy of NHz is 192.45 JK+mol-1 at 298K, and its heat capacity is given by the equation Com= a +bT +c/T2 with the coefficients given in the table below. Calculate the standard molar entropy of NH3 at 100 °C. Please explain as much as possible. Why did you use the equation? Or what conditions did you see from the question? etc. Table 1: Temperature variation of molar heat capacities, Cp /K-mol-?) = a +bT + c/T2 b/(10-3K-1)...
1. a) Calculate the change in entropy (AS) when one mole of diamond is heated from a temperature of 0 K to 400 K at a constant pressure of 1 bar. The temperature-dependent heat capacity of diamond is C 2.9x10 T J/(mol K), where T is the absolute temperature in K. b) Given that the entropy of diamond is zero at 0 K, calculate its absolute molar entropy (S) at 400 K from the above result.
The standard molar entropy of NH3 is 192.45 J K'mol ' at 298 K, and its heat capacity is given by the equation Cp.m = a + bT + c/T2 with the coefficients given in table below. Calculate the standard molar entropy of NH3 at a) 100 °C. (10 pts) Table 1: Temperature variation of molar heat capacities, C /OK-Imol-1) = a +bT + c/T2 c b/(10-K) I 25.1 /(10% K) -155 NH3 29.75
Question 20 Calculate the heat capacity, the molar heat capacity and the specific heat of a 16g sample of KOH, if it gives off 200kJ of heat and has an initial temperature of 25°C and a final temperature of 41°C.
The constant-pressure molar heat capacity of H2O (s) and H2O (l) is 75.291 J K−1 mol−1 and that of H2O (g) is 33.58 J K−1 mol−1 . Assume that the constant-pressure molar heat capacities are constant over the studied temperature range. Calculate the change in entropy of the system when 15.0 g of ice at −12.0 °C is converted to water vapour at 105.0 °C at a constant pressure of 1 bar!
Calculate the molar heat capacity of iron, A 45.61g piece of iron heated to 96.32˚C is transferred to a calorimeter containing 80.00g water initially at 24.91˚C. The temperature of the system at thermal equilibrium is 28.04˚C.
Estimate the molar entropy of potassium chloride at 5 Kelvin given that its molar heat capacity at that temperature is 1.2 microjoules per Kelvin x Mole. The answer is 4.0x10^-4 Joules per Kelvin Mole but I don't know how they got that answer.
The molar heat capacity at constant pressure Cp,m of certain ideal gas was found to vary according to the expression Cp,m = co + ciT, where co = 6.723 J K-1 mol-1 and cı = 0.1222 J K-2 mol-1 are constants peculiar to the gas. Calculate q, w, AU, and AH for a system comprising 3.0 mol of the gas undergoing the following reversible transformations: (a) the temperature of the gas is raised from 25.00°C to 100°C at constant pressure....