The standard enthalpy of formation of NH_2(g) id -46 KJ mol^-1.The standard enthalpy of formation of...
4. The standard enthalpy of formation of NH3 (g) is -46.11 kJ mol-' at 298 K. Given the heat capacity data below and the data in Problem 2, calculate the standard enthalpy of formation at 1200 K Cp.m (H2 (9))/ J mol K-1 = 29.1 - (0.84 x 10- K-)T Cpm (N2 (g))/ J mol K-1 = 26.98 +(5.9 x 10-'K-!)T
The standard molar enthalpy of combustion, deltacHm, of C2H6 (g) is -1559.8 kJ/mol. 1. Use some of the following data to calculate the molar enthalpy of formation of C2H6(g) at 298.15 K 2. Calculate the molar enthalpy of combustion of ethane at 500K Table provided gives values of standard enthalpy of formation values at 298.15 K Substance deltafH (kJ*mol^-1) Cpm (J*K^-1*mol^-1) CO2 (aq) -413.8 N/A CO2 (g) -393.51 37.11 H2O (l) -285.83 75.291 H2O(g) -241.82 33.58 C2H6(g) to be determined...
The standard enthalpy of combustion of cyclopropane is -2091 kJ/mol at 298 K. The enthalpy of formation of CO_2 (g) and H_2 O (I) are -393 kJ/mol and -286 kJ/mol, respectively. Calculate the enthalpy of formation of cyclopropane Given that the enthalpy of formation of propene is 20.42 kJ/mol, please calculate the enthalpy of isomerization of cyclopropane to propene.
The standard enthalpy of formation of NaF(s) is -573.6 kJ/mol, and the standard enthalpy of formation of NaF(aq, 1m) is -572.8 kJ/mol. Determine the standard enthalpy of solution of NaF.-0.8 kJ/mol-572.0 kJ/mol+0.8 kJ/mol-1146.4 kJ/mol+1146.4 kJ/mol
1) The standard enthalpy and free energy of formation ofH,O(g) arc -241.8 kJ/mol and-228.8 kJ/mol, respectively. What will be the AG of the following reaction at 100 °CifASis NOT independent of tcmpcraturc? State any assumption(s) you may need for the calculation. 2 H.(g)+0(g)2HO (8) △6873ド) (You may need the following: at 25°C the molar hcat capacity of gascous water is 33.76 J K1 mol at constant pressure; for the diatomic gas H2 and O;, the molar C (5/2)R.)
A scientist measures the standard enthalpy change for the following reaction to be 60.3 kJ: co_2(G) + h_2 (G) rightarrow CO(g) + H_2O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO_2(g) is kJ/mol.
3. (14 pts.) The standard molar enthalpy of formation of Fe,Oxs is AH = -8242 kJ/mol, and the standard molar enthalpy of formation of SO2(g) is AH = -296.8 kJ/mol (both at 298 K). Use this information, along with the standard molar enthalpy change of the following reaction at 298K, 2 FeS21s) + 11/2O2(g) → Fe2O3 + 4 SO2(g) AH = -1655 kJ/mol To determine the standard molar enthalpy change of the reaction shown below are 298 K: Fe(s) +...
The following table lists some enthalpy of formation values for selected substances. Substance ΔfH∘ΔfH∘ (kJ mol−1)(kJ mol−1) CO2(g)CO2(g) −393.5−393.5 Ca(OH)2(s)Ca(OH)2(s) −986.1−986.1 H2O(l)H2O(l) −285.8−285.8 CaCO3(s)CaCO3(s) −1207−1207 H2O(g)H2O(g) −241.8−241.8 Part A: Determine the enthalpy for this reaction: Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l) C a ( O H ) 2 ( s ) + C O 2 ( g ) → C a C O 3 ( s ) + H 2 O ( l ) Express your answer in kJ mol−1 k J m o l...
1. (14 pts) Determine the standard molar enthalpy of formation of B2He (g) at 298 K using only the data below. The standard state of boron at 298 K is a crystalline solid, B(s). AH-2368 kJmol а) 2B (5) B,0, (s) AH-1941 kJ/mol 3H.O (g) +30, (e) B O, (s) 2) В,н, @ AH-242 kJmol но (3) H, (g) +
The standard enthalpy of formation of CO(g) is −111 kJ/mol [refer to this equation C(s) + 1/2O2(g) ⟶ CO(g)] What is the ΔHorxn of this reaction? (What is the standard enthalpy change of this reaction?) 2C(s) + O2(g) ⟶ 2CO(g) -253 kJ/mol - 222 kJ/mol -97.1 kJ/mol 534 kJ/mol 124.9 kJ/mol -50.5 kJ/mol 5 points QUESTION 2 (assume A, B, C, and D and E are chemicals) Look at these equations A + B à C ΔH° = -9 kJ/mol rxn...