Consider the following reaction at 298 K and calculate the
following quantities:
dS system = S° product - S° reactant
dS system = S° 2x Al2O3 - [ S° 3 x O2 + S° 4 x Al]
dS system = 2 x 50. 92 - [ 3 x 205.03 + 4 x 28.33]
dS system = 101.84 - [ 615.09 + 113.32]
dS system = -626.57 J/mol.K
dS surr = - dH /T => -(-3351.4 kJ/mol / 298 K)
dS surr = 11.246 kJ/mol.K or 11246 J/mol.K
dS univ = dS system + dS surr
dS univ = - 626.57 + 11246 => 10619 J/mol.K
Consider the following reaction at 298 K and calculate the following quantities: Consider the following reaction...
Consider the following reaction at 298 K: 2Al(s) + 3Cl_2 (g) rightarrow 2AlCl_3(s) delta H degree = -1408.4 kJ Calculate the following quantities. Find standard entropy values
Consider the following reaction at 298 K. 4Al(s)+3O2(g)⟶2Al2O3(s) Δ?∘=−3351.4 kJ Calculate the following quantities. Refer to the standard entropy values as needed. Δ?sys= J/K Δ?surr= J/K Δ?univ= J/K Al Entropy = 28.3 O2 Entropy=205.2 Al2O3= 50.9
Calculate the standard enthalpy change for the following reaction 2Al_2O_3(s) + 3C(s) rightarrow 4Al + 3CO_2(g) given the following: delta H CO_2(g) = -393.5 kJ/mol delta H C(s) = 0 kJ/mol delta H Al = 10.79 kJ/mol delta H Al_2O_3(s) = -1675.7 kJ/mol
Consider the reaction 2NO_2(g) rightarrow N_2O_4 (g). Using the following data, calculate Delta G degree at 298 K. Delta G degree (NO_2(g)) = 51.84 kJ/mol, Delta G degree (N_2 O_4 (g)) = 98.28 kJ/mol. Calculate Delta G at 298 K if the partial pressures of NO_2 and N_2O_4 are 0.37 atm and 1.62 atm, respectively. Express your answer using one significant figure.
Given the following thermochemical equation: 2 Al + Fe_2O_2 rightarrow Al_2O_2 + 2Fe delat H = - 852 kJ What is Delta H when 0.100 mal of Al_2O_3 react with 0.250 mol of Fe? _____ kJ Using the data from Appendix G of the textbook, calculate Delta H for the combustion of 1.00 mole of C_2H_5OH(l). Note that (g) or (l) after the chemical formula denotes whether the compound is a gas or liquid. Some compounds have entries for both....
Calculate the value of K, at 298 K, for each value of delta G degree. delta G degree = 7.5 kJ/mol delta G degree = -9.0 kJ/mol
Consider the following reaction at 298 K: C(graphite) + 2CI2(g)→ CCI4(l) ΔH°=-139 kJ Calculate the following quantities.
What is the change in the internal energy of a system (delta U) if 71 kJ of heat energy is absorbed by the system and 12 kJ of work is performed on system? Write a balanced thermochemical equation for the following process: If 2 mol of sodium metal reacts with 1 mol of fluorine gas at constant pressure, 2 mol of solid sodium fluoride is produced and 409.2kJ of heat is released. How much energy is released if one mole...
Consider the following reaction at 298 K 2 Al(s) + 3 C12(E) — 2 AICI,() Calculate the following quantities. Refer to the standard entropy values as need Calculate the AS98 = Assurr = Suniv TOOLS x10
Consider the reaction at 298 K. C(graphite)+2 H 2 (g)⟶ CH 4 (g)Δ?°=−74.6 kJ C(graphite)+2H2(g)⟶CH4(g)ΔH°=−74.6 kJ Calculate the quantities. Delta Ssys=_______ J/K Delata Ssurr =_______ J/K