Given these reactions, where X represents a generic metal or metalloid 1) H2(g)+12O2(g)⟶H2O(g)Δ?1=−241.8 kJ1) H2(g)+12O2(g)⟶H2O(g)ΔH1=−241.8 kJ...
Given these reactions, where X represents a generic metal or metalloid
1) H2(g)+12O2(g)⟶H2O(g)Δ?1=−241.8 kJ1) H2(g)+12O2(g)⟶H2O(g)ΔH1=−241.8 kJ
2) X(s)+2Cl2(g)⟶XCl4(s)Δ?2=+157.3 kJ2) X(s)+2Cl2(g)⟶XCl4(s)ΔH2=+157.3 kJ
3) 12H2(g)+12Cl2(g)⟶HCl(g)Δ?3=−92.3 kJ3) 12H2(g)+12Cl2(g)⟶HCl(g)ΔH3=−92.3 kJ
4) X(s)+O2(g)⟶XO2(s)Δ?4=−769.5 kJ4) X(s)+O2(g)⟶XO2(s)ΔH4=−769.5 kJ
5) H2O(g)⟶H2O(l)Δ?5=−44.0 kJ5) H2O(g)⟶H2O(l)ΔH5=−44.0 kJ
what is the enthalpy, Δ?,ΔH, for this reaction?
XCl4(s)+2H2O(l)⟶XO2(s)+4HCl(g)
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Given these reactions, where X represents a generic metal or
metalloid
1) H2(g)+12O2(g)⟶H2O(g)Δ?1=−241.8 kJ1)
H2(g)+12O2(g)⟶H2O(g)ΔH1=−241.8 kJ...
Consider these reactions, where M represents a generic metal. 2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−600.0 kJ HCl(g)⟶HCl(aq) ΔH2=−74.8 kJ H2(g)+Cl2(g)⟶2HCl(g) ΔH3=−1845.0 kJ...
Consider these reactions, where M represents a generic metal. 2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−600.0 kJ HCl(g)⟶HCl(aq) ΔH2=−74.8 kJ H2(g)+Cl2(g)⟶2HCl(g) ΔH3=−1845.0 kJ MCl3(s)⟶MCl3(aq) ΔH4=−215.0 kJ Use the given information to determine the enthalpy of the reaction 2M(s)+3Cl2(g)⟶2MCl3(s) ΔH= kJ
Given these reactions, where X represents a generic metal or metalloid 1)H,(8) + 402(8) — 4,0(8)...
Given these reactions, where X represents a generic metal or metalloid 1)H,(8) + 402(8) — 4,0(8) 2) X(s) + 2 C12(g) → XCI_(5) 3) {H_(9) + Cl2(9) — HCI(9) AH = –241.8 kJ AH2 = +255.5 kJ AHz = -92.3 kJ 4) X(s) + O2(g) → XO_(s) AH4 = -753.1 kJ 5) H2O(g) — H2O(1) AH3 = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI_(s) + 2 H2O(l) → XO2 (s) + 4 HCI(g) AH =
Consider these reactions, where M represents a generic metal. 2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)Δ?1=−924.0 kJ2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−924.0 kJ HCl(g)⟶HCl(aq) Δ?2=−74.8 kJHCl(g)⟶HCl(aq) ΔH2=−74.8 kJ H2(g)+Cl2(g)⟶2HCl(g).
Consider these reactions, where M represents a generic metal. 2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)Δ?1=−924.0 kJ2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−924.0 kJ HCl(g)⟶HCl(aq) Δ?2=−74.8 kJHCl(g)⟶HCl(aq) ΔH2=−74.8 kJ H2(g)+Cl2(g)⟶2HCl(g) Δ?3=−1845.0 kJH2(g)+Cl2(g)⟶2HCl(g) ΔH3=−1845.0 kJ MCl3(s)⟶MCl3(aq) Δ?4=−123.0 kJMCl3(s)⟶MCl3(aq) ΔH4=−123.0 kJ Use the given information to determine the enthalpy of the reaction 2M(s)+3Cl2(g)⟶2MCl3(s)
Given these reactions, where X represents a generic metal or metalloid 1) H,(g) + 0,(g) –...
Given these reactions, where X represents a generic metal or metalloid 1) H,(g) + 0,(g) – HO(g) AH = -241.8 kg 2) X(s) + 2 C1,(8) XCI(S) AH = +182.9 kJ 3) H,(8) + CI,(E) — HCI(8) AH; = -92.3 kJ 4) X(8) + 0,(8) — X0,() AHA = -756,5 kJ 5) H.O(g) - HO(1) AHS = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI,(s) + 2 H,001) — XO,(s) + 4 HCl(g) AH =
1) C2H6 (g) -----> C2H4 (g) + H2 (g) ΔH1 = ? 2) C2H6 (g) +...
1) C2H6 (g) -----> C2H4 (g) + H2 (g) ΔH1 = ? 2) C2H6 (g) + 3.5O2 (g) -----> 2CO2 (g) + 3H2O (l) ΔH2 = -1560 kJ/mo 3) C2H4 (g) + 3O2 (g) -----> 2CO2 (g) + 2H2O (l) ΔH3 = -1411 kJ/mol 4) 2H2O (l) -----> 2H2 (g) + O2 (g) ΔH4 = 571.6 kJ/mol How much heat is transferred between the system and the surroundings when 25 grams of ethane (C2H6) decomposes to produce ethylene (C2H4) and...
Consider these reactions, where M represents a generic metal.2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−869.0kJHCl(g)⟶HCl(aq)ΔH2=−74.8kJH2(g)+Cl2(g)⟶2HCl(g)ΔH3=−1845.0kJMCl3(s)⟶MCl3(aq)ΔH4=−477.0kJUse the given information to determine the enthalpy...
Consider these reactions, where M represents a generic metal.2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−869.0kJHCl(g)⟶HCl(aq)ΔH2=−74.8kJH2(g)+Cl2(g)⟶2HCl(g)ΔH3=−1845.0kJMCl3(s)⟶MCl3(aq)ΔH4=−477.0kJUse the given information to determine the enthalpy of the reaction2M(s)+3Cl2(g)⟶2MCl3(s)
Given the reactions, X(s)+12O2(g)⟶XO(s)Δ?=−983.5 kJX(s)+12O2(g)⟶XO(s)ΔH=−983.5 kJ XCO3(s)⟶XO(s)+CO2(g)Δ?=+253.5 kJXCO3(s)⟶XO(s)+CO2(g)ΔH=+253.5 kJ what is Δ? for this reaction? X(s)+12O2(g)+CO2(g)⟶XCO3(s)
Given the reactions, X(s)+12O2(g)⟶XO(s)Δ?=−983.5 kJX(s)+12O2(g)⟶XO(s)ΔH=−983.5 kJ XCO3(s)⟶XO(s)+CO2(g)Δ?=+253.5 kJXCO3(s)⟶XO(s)+CO2(g)ΔH=+253.5 kJ what is Δ? for this reaction? X(s)+12O2(g)+CO2(g)⟶XCO3(s)
Given the following reactions: 2 S (s) + 3 O2 (g) ⟶ 2 SO3 (g) ΔH1= LaTeX: -− 790 kJ S (s) + O2 (g) ⟶ SO2 (g) ΔH2= LaTeX:...
Given the following reactions: 2 S (s) + 3 O2 (g) ⟶ 2 SO3 (g) ΔH1= LaTeX: -− 790 kJ S (s) + O2 (g) ⟶ SO2 (g) ΔH2= LaTeX: -−297 kJ What is the enthalpy change of the following reaction? 2 SO3 (g) ⟶ 2 SO2 (g) + O2 (g) ΔH3=?
24. Consider the combustion of hydrogen given below H2(g) + ½Og(g) H2O(g) ΔH =-241.8 kJ/mol →...
24. Consider the combustion of hydrogen given below H2(g) + ½Og(g) H2O(g) ΔH =-241.8 kJ/mol → What is the enthalpy change, in kJ, when the reaction is started with 52.5 g of H2 and 52.5 g of O2? A) -793 kJ B) -537 k C) -192 k D) -645 kJ E) 564 kl
Consider the following reaction 4HCl(g) + O2(g) 2H2O(g) + 2Cl2(g) HCl(g) H2O (g) Hof (kJ/mol) -...
Consider the following reaction 4HCl(g) + O2(g) 2H2O(g) + 2Cl2(g) HCl(g) H2O (g) Hof (kJ/mol) - 92.3 - 241.8 Gof (kJ/mol) - 75.3 - 228.6 a) (12 pts) Predict which direction, forward or reverse, is accompanied by increasing disorder (Show your calculations). b) (3 pts) Can this reaction be reversed by changing the temperature? Explain. c) (3 pts) Calculate Kp for the above reaction at 25oC? d) (5 pts) Calculate the free energy, G, for the above reaction at 200C...
Given these reactions, where X represents a generic metal or metalloid 1)H,(8) + 402(8) — 4,0(8) 2) X(s) + 2 C12(g) → XCI_(5) 3) {H_(9) + Cl2(9) — HCI(9) AH = –241.8 kJ AH2 = +255.5 kJ AHz = -92.3 kJ 4) X(s) + O2(g) → XO_(s) AH4 = -753.1 kJ 5) H2O(g) — H2O(1) AH3 = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI_(s) + 2 H2O(l) → XO2 (s) + 4 HCI(g) AH =
Given these reactions, where X represents a generic metal or metalloid 1) H,(g) + 0,(g) – HO(g) AH = -241.8 kg 2) X(s) + 2 C1,(8) XCI(S) AH = +182.9 kJ 3) H,(8) + CI,(E) — HCI(8) AH; = -92.3 kJ 4) X(8) + 0,(8) — X0,() AHA = -756,5 kJ 5) H.O(g) - HO(1) AHS = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI,(s) + 2 H,001) — XO,(s) + 4 HCl(g) AH =
24. Consider the combustion of hydrogen given below H2(g) + ½Og(g) H2O(g) ΔH =-241.8 kJ/mol → What is the enthalpy change, in kJ, when the reaction is started with 52.5 g of H2 and 52.5 g of O2? A) -793 kJ B) -537 k C) -192 k D) -645 kJ E) 564 kl
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