The equation Cp,m = a + bT + c/T2
This equation is use because heat capacity is varies with change in temperature is large amount, Normally we neglect heat capacities changes with small variation in temperature. This equation is use where your compound is more effective or responsive with temperature.
The standard molar entropy of NHz is 192.45 JK+mol-1 at 298K, and its heat capacity is...
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 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 entropy change of the following reaction (in JK) the following standard entropy values (given in J/mol-K): A-2922, B-2424. C-2618, D = Number J/K
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.
a) calculate the standard reaction entropy (in J K-1 mol-1) at 298K for the complete combustion of sucrose. b) Calculate the standard Gibbs reaction energy (in kJ mol-1) for the reaction
Physical Chemistry Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol K1 and 31.75 J mol K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g1. The molar mass of aluminum is...
The molar heat capacity Cp m of SO2 (g) is described by the following equation over the range 300 K< T < 1700 K 45.81 x 10-7 T2 ка Cp +1.035 x 10-9 Ț3. кз 3.093 6.967 x 10-3 In this equation, T is the absolute temperature in kelvin. The ratios T"/K" ensure that Cp.m has the correct dimension. 1.65 moles of SO2 (g) is heated from 29.0 C to 1130 ° C at a constant pressure of 1 bar
C(graphite) +2H2g) CH4(g) A,H (298K)74.87 kI mol- 5. Calculate the standard heat for combustion for ethylene: C2H(g) +202(g) 2CO2(g)+ 2H20(9). by using the following standard heat of formation C,H (g) 2CGgraphite) + 2H,(@). a, (29k) 52 kj mol-, Co(g) C(graphite) + Op(g). 4,Ho (298k)--394 k3 mol and H0C) Hea)+0,(g) 4(98K)- -242 k mol
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.
A reaction has an enthalpy change of - 71 kJ mol" and an entropy change of -58 JK-mol-. At what temperature does this exothermic reaction cease to be spontaneous? 422°C 673°c 826°C O 951°C What is the molar reaction enthalpy for the reaction below: N2H4(0) +CHNO(0) 4CHẠO(g) +Ng(g) + 3H (g) given the following thermodynamic data? 2NH3(9) ► N2H4(l) + H2(9) A,Hm = 22.5 kJ mol-1 2NH3(9) N2(g) + 3H2(9) A Hm = 57.5 kJ mol-1 CH,0(9) + H2(g) +...