The molar heat capacity Cp m of SO2 (g) is described by the following equation over...
Please help me solve for delta H, I can't get it. Thank you! Part A Constants | Periodic Table The molar heat capacity Cp,m of SO2 (g) is described by the following equation over the range 300 K
The molar heat capacity of SO2(g) changes with temperature, and is approximately described by the following equation: Cp,M/R = 3.093 + (6.967 x 10-3 K-1)T In this equation, T is the absolute temperature in kelvin (K). The K-1 ensures that Cp,M has the correct dimensions. Assuming ideal gas behavior, calculate q and delta H if 1.5 mol of SO2(g) is heated from 25o C to 1140o C at a constant pressure of 1 bar. Explain the sign of q.
The temperature dependence of the molar heat capacity at constant pressure for Cl_2(g) in the temperature range from 298-800 K is: C_p, m(J mol^-1 K^-1) = 22.85 - 0.06543T - (1.2517 times 10^-4)T^2 + (1.1484 times 10^-7)T^3 Where T is the Kelvin temperature. Calculate the heat required to raise the temperature of 1.000 mole of Cl_2(g) from 300 K to 800 K.
5. (20 pts.) The molar heat capacity CP.m of H2O(g) from 373 K to 473 K at a constant pressure of 1 atm is Cp,l = 30.54 +(1.03x10-2T) where the units of Cp.m are JK mol!. a) (10 pts.) Calculate AH if 1 mol of H20 (g) is heated from 373 to 473 K at a constant pressure of 1 bar. b) (10 pts.) Calculate AU for the same thermodynamic change of state. Assume ideal gas behavior to do this...
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
The molar heat capacity of ethene gas can be expressed by over the temperature range 300 K < T < 1000 K. Calculate AS if one mole of ehtene is heated from 300 K to 600 K at constant volume. b) Using the data from part a) and assuming ideal behavior such that Cp_m - CV_m=R, calculate AS if one mole of ethene is heated from 300 K to 600 K at constant pressure.
1. At 10K the molar heat capacity of gold is 0.43 J K-1 mol-1. Ass ume that termine the Cp of gold varies as CP = aT over the range 0 to 10K. De entropy at 10K assuming that S(T 0-0.
- 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 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....
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)...