Solution:
Part A : Delta H0rxn = 88 kJ
Delta Srxn = 155 J / K,
T = 307 K
We have to calculated delta S of universe:
Delta H of universe = delta S of system + delta S of surrounding.
Delta of surrounding = - delta H / T
= - 88000 J / 307 K
= -286.645 J/K
Lets plug this value in above equation.
Delta S universe = [155 J + (-286.645) ] J/K
=-131.65 J/K
Part B :
Here we use same equation only T is changed.
Delta of surrounding = - delta H / T
= - 88000 J / 758 K
=- 116.095 J / K
Lets plug this value
Delta S universe = 155 + (-116.094) J / K = 38.905 J/K
Given the values of DeltaH degree_rxn, DeltaS degree_rxn, and T below, determine DeltaS_univ.
Using the accepted values of deltaH and deltaS, calculate ksp of anhydrous CaSO4 at 5 degrees C. Accepted values---- DeltaS -139.7 J/mol K, Delta H -18.99 kJ/mol
Ag2S given DeltaH= -32 kj/mol, DeltaG=-40 kj/mol DeltaS= 146 j/k*mol calculate Gibbs free energy for the reaction of dissolving silver sulfide, Ag2S, in water (25 C.) Do the calculations in two ways. Use the standard Enthalpy of formation, deltaH, and entropy S values, and the formula deltaG=deltaH-TdeltaS. Use the standard free energies of formation deltaG and the formula deltaG=deltaG(products)-deltaG(reactants).
Given reactions 1 and 2 below, calculate delta H degree_Rxn and delta U degree_Rxn for reaction 3. Rxn 1 H_2(g) + I_2(s) rightarrow 2 HI(g) delta H degree_Rxn = +52.96 kJ/mol Rxn 2 2H_2(g) + O_2(g) rightarrow 2 H_2 O(g) delta H degree_Rxn = -483.64 kJ/mol Rxn 3 4 HI(g) + O_2(g) rightarrow 2 I_2(s) + 2 H_2O(g) delta H degree_Rxn = ? delta U degree_Rxn = ?
Consider the decomposition of CaCO3 at standard conditions: CaCO3(s) >> CO2(g) + CaO(s) DeltaH=177.8 KJ/mol, DeltaS=160.5 J/K mol, DeltaG=130.3 KJ/mol, K=1.506x10^-23, Nonspontaneous until temp 1107.8 K or higher. What is the new concentration of CO2 at nonstandard temperature (1107.8k)?
Consider the decomposition of CaCO3 at standard conditions: CaCO3(s) >> CO2(g) + CaO(s) DeltaH=177.8 KJ/mol, DeltaS=160.5 J/K mol, DeltaG=130.3 KJ/mol, K=1.506x10^-23, Nonspontaneous until temp 1107.8 K or higher. What is the new concentration of CO2 at nonstandard temperature (1107.8k)?
Given the values of AHrxn, ASrxn, and T below, determine AS univ. Part A AHIX = 124 kJ , ASIX = – 248 J/K , T = 292 K.
Determine Delta S degree_rxn for H_2 (g) + I_2 (g) 2 HI (g) given the following information: a. -41.10 J/K b. 398.75 J/K c. -165.29 J/K d. + 41.10 J/K e. + 165.29 J/K
Given the values of ΔHorxn, ΔSorxn, and T below, determine ΔSuniv. ΔHorxn= -95 kJ , ΔSorxn= -157 J/K , T= 855 K (HINT: Use the equation on page 876, ΔSuniv = ΔS - ΔH / T ). Group of answer choices -45.9 J/K -111.1 J/K -157 J/K +238.7 J/K -268.11 J/K
Use the delta H degree information provided to determine delta H degree_rxn for the following reactions: CH_4(g) + 3 Cl_2(g) rightarrow CHCl_3(l) + 3 HCl(g) delta H degree_rxn = ? CH_4(g) = -75 kJ/mol; CHCl_3(l) = -134 kJ/mol; HCl(g) = -923 kJ/mol
Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv and whether they are spontaneous or nonspontaneous: A. ΔH∘rxn= 80 kJ , ΔSrxn= 143 J/K , T= 290 K B. ΔH∘rxn= 80 kJ , ΔSrxn= 143 J/K , T= 764 K C. ΔH∘rxn= 80 kJ , ΔSrxn=− 143 J/K , T= 290 K D. ΔH∘rxn=− 80 kJ , ΔSrxn= 143 J/K , T= 396 K