Without doing any calculations, determine the sign of ΔSsys and ΔSsurr for each of the chemical reactions below. Part A 2CO(g)+O2(g)⇌2CO2(g)ΔH∘rxn= -566.0 kJ -566.0 ΔSsys>0, ΔSsurr>0 ΔSsys<0, ΔSsurr>0 ΔSsys>0, ΔSsurr<0 ΔSsys<0, ΔSsurr<0 SubmitMy AnswersGive Up Part B 2NO2(g)→2NO(g)+O2(g)ΔH∘rxn= +113.1 kJ +113.1 ΔSsys>0, ΔSsurr>0 ΔSsys<0, ΔSsurr>0 ΔSsys>0, ΔSsurr<0 ΔSsys<0, ΔSsurr<0 SubmitMy AnswersGive Up Part C 2H2(g)+O2(g)→2H2O(g)ΔH∘rxn= -483.6 kJ -483.6 ΔSsys>0, ΔSsurr>0 ΔSsys<0, ΔSsurr>0 ΔSsys>0, ΔSsurr<0 ΔSsys<0, ΔSsurr<0
Since a) 2CO(g)+O2(g)⇌2CO2(g)
In this reaction, ΔH∘rxn= -566.0 kJ which means reaction is exothermic. So, heat flows from system to surroundings.So, ΔSsurr>0.Not only that 3 molecules of reactants give two molecules of product. Therefore, there is reduction in degree of freedom of the system i.e. ΔSsys<0
Since, ΔSsys + ΔSsurr > 0, therefore , ΔSsys<0, ΔSsurr>0
b) 2NO2(g)→2NO(g)+O2(g)
For this reaction, ΔH∘rxn= +113.1 kJ i.e. the reaction is endothermic. So, heat flows from surroundings to system. Thus, ΔSsurr<0. Not only that 2 molecules of reactants give 3 molecules of product. Therefore, there is increase in degree of freedom of the system , that makes ΔSsys>0.
Since, ΔSsys + ΔSsurr > 0,Therefore, ΔSsys>0, ΔSsurr<0
c) 2H2(g)+O2(g)→2H2O(g)
For this reaction, ΔH∘rxn= -483.6 kJ i.e exothermic.
So, heat flows from system to surroundings.So, ΔSsurr>0.Not only that 3 molecules of reactants give two molecules of product. Therefore, there is reduction in degree of freedom of the system i.e. ΔSsys<0
Since, ΔSsys + ΔSsurr > 0, therefore , ΔSsys<0, ΔSsurr>0
Without doing any calculations, determine the sign of ΔSsys and ΔSsurr for each of the chemical...
Question 6 1.5 pts Predict under what temperatures (all temperatures, low temperatures, or high temperatures), if any, the following reactions will be spontaneous. A. 2CO(g) + O2(g) = 2002(g), AH rxn=-566.0 kJ [ Select] B. 2NO2(g)2NO(g)+O2(g), AH rxn= +113.1 kJ [ Select ] C. 2H2(g)+O2(g)—2H2O(g), AH rxn=-483.6 kJ [ Select] D. 2H2O2(1)→2H2O(1)+O2(g), AH rxn= -196.0 kJ [Select ]
Without doing any calculations, determine the sign of ΔSsysΔSsys for each of the following chemical reactions. Drag the appropriate items to their respective bins. Part A Without doing any calculations, determine the sign of ASsys for each of the following chemical reactions. Drag the appropriate items to their respective bins. Reset Help + CH=CH(g) + H2(g)→ CH2=CH2(g) 2NO(g) + O2(g) +2NO2(g) 4Li(s) + O2(g) +2Li20(s) 2KMnO4(s)→ K2MnO4(s) + MnO2(s) + O2(g) ASsys > 0 ASsys < 0
Part A Calculate Δ Han for the following reaction: C(s) +H2O(g)CO(g)+H2() Use the following reactions and given ΔΗ values: C(s) + O2 (g)- CO2 (g), ΔΗ-393.5 kJ 2CO (g) + O2 (g)--2CO2 (g), ΔΗ-566.0 kJ 2H2 (g) +02 (g)-2H3O(g). Ан :-483.6 kJ Express your answer using four significant figures. kJ Submit Request Answer
0.75 pts Without doing any calculations, determine the sign of ASsys for each of the following chemical reactions A. 2KCIOg(s)-2KCI(s)+3O2(g) [Select ] B. C(s)+2H2(g)→CH4(g) [ Select ] C. Na(s)+1/2 Cl2(g)-NaCl(s) [ Select ] D. N2(g)+3H2(g)→2NH3(g) [Select ]
Q Searc Without doing any calculations, match the following thermodynamic properties with their appropriate numerical sign for the following exothermic reaction. 2CO(g) + O2(g) +2CO2(g) Clear All > 0 Ангол <0 ASTA AGEN > low T, <0 high T AS universe <0 low T. >O high T Regenerate Group 10. Qualitative Delta G, H, S: This is group attempt 1 of 5 References Use the References to access important values if needed for this question. For the reaction 2002(g) +...
----------- ------------ Without doing any calculations, match the following thermodynamic properties with their appropriate numerical sign for the following endothermie reaction 2co2(e)+N2(e2co+2NO) Clear All 3 0 s 0 ASuniverse >0 low T,0 high T 0 low T,>0 highT
Without doing any calculations, match the following thermodynamic properties with their appropriate numerical sign for the following endothermic reaction. CH4(g) + H2O(g) +CO(g) + 3H2(g) Clear All >0 AGX <0 ASPX 0 AS universe > 0 low T, <0 high T ΔΗχη <0 low T,> 0 high T 10. Qualitative Delta G, H, S: This is group attempt 1 of 5 Without doing any calculations, match the following thermodynamic properties with their appropriate num sign for the following endothermic reaction....
Part A Use standard free energies of formation to determine AG for this reaction at 25° C. rxn Express the free energy change to four significant figures and include the appropriate units. ? kJ AG Value rXn mol Request Answer Previous Answers Submit XIncorrect; Try Again; 5 attempts remaining You may want to reference (Page) Section 18.8 while completing this problem. G One of the reactions that occurs within a catalytic converter in the exhaust pipe of a car is...
Without doing any calculations, determine the sign of ∆H for each chemical reaction:a) NaNO3(s)→Na+(aq)and NO3-(aq)b) the freezing of liquid waterc) CaCO3(s)→CaO(s)+ CO2(g)
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...