Given the reactions below, answer the following questions. Cl2(g) + F2(g) = 2ClF(g) $\Delta G_{\text{rxn}}^\circ$ =...

Question

Question

Given the reactions below, answer the following questions.

Cl2(g) + F2(g) = 2ClF(g) $\Delta G_{\text{rxn}}^\circ$ = 115.4 kJ/mol

Cl2(g) + Br2 (g) =2ClBr(g) $$ $\Delta G_{\text{rxn}}^\circ$ = –2.0 kJ/mol

Calculate the Δ?∘rxn for

2ClF(g) +Br2(g) = 2ClBr(g) + F2(g)

Answer 1

Answer #1

Cl2(g) + F2(g) = 2ClF(g) Δ?∘ = 115.4 kJ/mol

Cl2(g) + Br2 (g) =2ClBr(g) Δ?∘ = –2.0 kJ/mol

Cl2(g) + F2(g) = 2ClF(g) Δ?∘ = 115.4 kJ/mol subtract two equations

(-) (-) (-) (-)

--------------------------------------------------------------------------------------------------

2ClF(g) +Br2(g) -------->2ClBr(g) + F2(g) Δ?∘rxn = -117.4KJ/mole >>>>>answer

Answer 2

Similar Homework Help Questions

Please answer this question Given the reactions below, answer the following questions. Cl_2(g) + F_2(g) rlhar...

Please answer this question Given the reactions below, answer the following questions. Cl_2(g) + F_2(g) rlhar 2ClF(g) delta G degree_rxn = 115.4 kJ/mol Cl_2(g) + Br_2(g) rlhar 2ClBr(g) delta G degree_rxn = -2.0 kJ/mol Calculate the delta G degree_rxn for 2ClF(g) + Br_2(g) rlhar 2ClBr(g) + F_2(g) __________ kJ/mol
Calculate the LaTeX: \Delta Δ G°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) LaTeX:...

Calculate the LaTeX: \Delta Δ G°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) LaTeX: \longrightarrow ⟶ 7 N2(g) + 12 H2O(l) LaTeX: \Delta Δ G°rxn = ? LaTeX: \Delta Δ G°f (kJ/mol) –73.5 149.3 –237.1
Given reactions 1 and 2 below, calculate delta H degree_Rxn and delta U degree_Rxn for reaction...

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 = ?

4) Given the thermochemical equations: (3 points) Br2(l) + F2(g) → 2BrF(g) Br2(1) + 3F2(g) →...

4) Given the thermochemical equations: (3 points) Br2(l) + F2(g) → 2BrF(g) Br2(1) + 3F2(g) → 2BrF3(g) AH°= -188 kJ/mol AH°= -768 KJ/mol Calculate the AH°rxn for the reaction BrF(g) + F2(g) → BrF3(9)
Reaction X: ½ I2 (s) + ½ Cl2 (g) → ICl (g) ∆Hºf,RXN = 18 kJ...

Reaction X: ½ I2 (s) + ½ Cl2 (g) → ICl (g) ∆Hºf,RXN = 18 kJ mol-1RXN, ∆Sº298 = 78 J K-1 mol-1 Reaction Y: ½ I2 (s) + ½ Br2 (l) → IBr (g) ∆Hºf,RXN = 41 kJ mol-1RXN, ∆Sº298 = 124 J K-1 mol-1 Calculate the value of the equilibrium constant, Keq, for reaction X at 25ºC.
Calculate the Delta H formation of N2O5 (g) given the below reactions: 2NO (g) + O2...

Calculate the Delta H formation of N2O5 (g) given the below reactions: 2NO (g) + O2 (g) -> 2NO2 (g), ΔHrxn = -114.1 kJ/mol 4NO2(g) + O2 (g) -> 2N2O5 (g), ΔHrxn = -110.2 kJ/mol N2 (g) + O2 (g) -> 2 NO (g), ΔHrxn = +180.5 kJ/mol

Use the standard reaction enthalpies given below to determine H°rxn for the following reaction: P4 (g) + 10 Cl2 (g)...

Use the standard reaction enthalpies given below to determine H°rxn for the following reaction: P4 (g) + 10 Cl2 (g) --> 4 PCl5 (s) ΔHreaction = ? Given: PCl5 (s) --> PCl3 (g) + Cl2 (g) ΔHreaction = +157 kJ P4 (g) + 6 Cl2 (g) --> 4 PCl3 (g) ΔHreaction = -1207 kJ Choices: A. -1835 kJ B. -1364 kJ C. -1050 kJ D. -1786 kJ E. -2100 kJ
Given: PCl5(s) → PCl3(g) + Cl2(g) ΔH°rxn = + 157 kJ

Given: PCl5(s) → PCl3(g) + Cl2(g) ΔH°rxn = + 157 kJ P4(g) + 6 Cl2(g) → 4 PCl3(g) ΔH°rxn = - 1207 kJ What is the standard-state enthalpy change for the following reaction? P4(g) + 10 Cl2(g) → 4PCl5(s)a -2100 kJb-1835 kJc-1364 kJD -1786 kJ
In which reactions is the AS rxn positive CIO(g) + O2(g) - CI(g) + 2O2(8) RXN...

In which reactions is the AS rxn positive CIO(g) + O2(g) - CI(g) + 2O2(8) RXN 01 203(g) 302(8) RXN 02 2 NO2(8) N204(8) RXN 03 RXN 02 only RXN 01 and RXN 02 RXN 01 only All three of the reactions None of the reactions RXN03 only RXN 02 and RXN 03 ORXN 01 and RXN03 - You have a process that is: Endothermic, Entropy decreases. Choose the best answer: O always non-spontaneous O spontaneous at high temperatures O...

Calculate AH® for the following: rxn CH4(g) + Cl2(g) → CCI_(1) + HCl(g) (unbalanced] NH (CH4()]...

Calculate AH® for the following: rxn CH4(g) + Cl2(g) → CCI_(1) + HCl(g) (unbalanced] NH (CH4()] = -74.87 kJ/mol AH (CC14(8)] =-96.0 kJ/mol AHCC140] =-139 kJ/mol AH [HCI(g)] = -92.31 kJ/mol AH [HCl(aq)] = -167.46 kJ/mol 1 - 121.0 kJ/mol kJ

Given the reactions below, answer the following questions. Cl2(g) + F2(g) = 2ClF(g) \(\Delta G_{\text{rxn}}^\circ\) =...