Assuming deltaH° and deltaS° are independent of temperature, calculate the temperature where K=1.00 for the following...
Assuming deltaH° and deltaS° are independent of
temperature, calculate the temperature where K=1.00 for the
following reaction
Fe2O3(s) + 3H2(g)----> 2Fe(s)+ 3H2O(g)
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Assuming deltaH° and deltaS° are independent of
temperature, calculate the temperature where K=1.00 for the
following...
Steps please. Assuming ΔΗο and AS"are independent of temperature, calculate the temperature where K- 1.00 for...
Steps please.
Assuming ΔΗο and AS"are independent of temperature, calculate the temperature where K- 1.00 for the following reaction: 5. Fe O3 (s) 3 H2(g) 2 Fe (s) + 3 H2O (g)
1. For the reaction: N2(g) + O2(g)=2NO(g), deltaH° = 181 kJ and deltaS° = 24.9 J/K,...
1. For the reaction: N2(g) + O2(g)=2NO(g), deltaH° = 181 kJ and deltaS° = 24.9 J/K, deltaG° would be negative at temperatures (above, below) ?????K. Enter above or below in the first box and enter the temperature in the second box. Assume that deltaH° and deltaS° are constant. 2. For the reaction: 2BrF3(g)=Br2(g) + 3F2(g), deltaH° = 542 kJ and deltaS° = 269 J/K, G° would be negative at temperatures (above, below) K. Enter above or below in the first box...
1.00 mol Fe(s) and 3.00 mol H2 (g) were placed into a 5.00 L reaction vessel...
1.00 mol Fe(s) and 3.00 mol H2 (g) were placed into a 5.00 L reaction vessel where the Kc for the reaction below is 0.825 at 400K. What is the concentration of hydrogen gas at equilibrium? Fe2O3 (s) + 3H2 (g) <----> 2Fe (s) + 3H2O (g)
11. For the reaction Fe2O3(s) + 3H2(g) +2Fe(s) + 3H2O(g) AH° = 98.8 kJ and AS°...
11.
For the reaction Fe2O3(s) + 3H2(g) +2Fe(s) + 3H2O(g) AH° = 98.8 kJ and AS° = 142.5 J/K The equilibrium constant for this reaction at 345.0 K is Assume that AHⓇ and AS are independent of temperature. For the reaction 2502(g) + O2(g) +2503(g) AH° = -197.8 kJ and AS° = -187.9 J/K The equilibrium constant for this reaction at 272.0 K is Assume that AH° and AS are independent of temperature.
1. Consider the reaction: H2CO(g) + O2(g)CO2(g) + H2O(l) Using standard absolute entropies at 298K, calculate...
1. Consider the reaction: H2CO(g) + O2(g)CO2(g) + H2O(l) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.41 moles of H2CO(g) react at standard conditions. S°system =___ J/K 2. For the reaction 3Fe2O3(s) + H2(g)>2Fe3O4(s) + H2O(g) DeltaH° = -6.0 kJ and DeltaS° = 88.7 J/K The standard free energy change for the reaction of 1.78 moles of Fe2O3(s) at 292 K, 1 atm would be ___ kJ. This reaction is (reactant, or product) favored...
Ag2S given DeltaH= -32 kj/mol, DeltaG=-40 kj/mol DeltaS= 146 j/k*mol calculate Gibbs free energy for the...
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).
1.) Calculate ΔHºrxn ΔSsurr and ΔSºrxn to determine if the reaction is spontaneous at 298 K ΔHºf...
1.) Calculate ΔHºrxn ΔSsurr and ΔSºrxn to determine if the reaction is spontaneous at 298 K ΔHºf : PCl3(g) = -287 kj/mol ΔSºf : PCl3(g) = -3112 J/mol *K ΔSºf : P4(s) = 41.1 J/mol*K ΔSºf : Cl2(g)= 2230 J/mol *K P4(s) +6Cl2(g) ------> 4PCl3(g) 2.) Calculate ΔGºrxn from enthalpy and entropy values at 298 K 4NH3 (g) +5O2(g) -----> 4 NO(g) +6H2O(g) ΔHºf : NO(g) = 90.29 kj/mol ΔHºf: H2O(g) = -241.826 kJ/mol ΔHºf: NH3(g) = -45.9 kJ/mol ΔSºf : NO(g)...
please help with these Fe2O3(s) + 3H2(g) +2Fe(s) + 3H2O(g) Using standard absolute entropies at 298K,...
please help with these
Fe2O3(s) + 3H2(g) +2Fe(s) + 3H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.37 moles of Fe2O3() react at standard conditions. AS system JK 2CO(g) + O2(g) +2CO2(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.54 moles of CO(g) react at standard conditions. AS system JK 2NH3(g) + 3N20(g)— 4N2(g) + 3H2O(g) AH = -879.5 kJ and AS° = 288.1 J/K The...
Consider the decomposition of CaCO3 at standard conditions: CaCO3(s) >> CO2(g) + CaO(s) DeltaH=177.8 KJ/mol, DeltaS=160.5...
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...
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)?
Steps please.
Assuming ΔΗο and AS"are independent of temperature, calculate the temperature where K- 1.00 for the following reaction: 5. Fe O3 (s) 3 H2(g) 2 Fe (s) + 3 H2O (g)
11.
For the reaction Fe2O3(s) + 3H2(g) +2Fe(s) + 3H2O(g) AH° = 98.8 kJ and AS° = 142.5 J/K The equilibrium constant for this reaction at 345.0 K is Assume that AHⓇ and AS are independent of temperature. For the reaction 2502(g) + O2(g) +2503(g) AH° = -197.8 kJ and AS° = -187.9 J/K The equilibrium constant for this reaction at 272.0 K is Assume that AH° and AS are independent of temperature.
please help with these
Fe2O3(s) + 3H2(g) +2Fe(s) + 3H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.37 moles of Fe2O3() react at standard conditions. AS system JK 2CO(g) + O2(g) +2CO2(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.54 moles of CO(g) react at standard conditions. AS system JK 2NH3(g) + 3N20(g)— 4N2(g) + 3H2O(g) AH = -879.5 kJ and AS° = 288.1 J/K The...
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