Consider the reaction 8H2S(g)+4O2(g)→8H2O(g)+S8(g)8H2S(g)+4O2(g)→8H2O(g)+S8(g) Δ[H2S]/ΔtΔ[H2S]/Δt = -0.022 M/sM/s You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. Part A Find Δ[O2]/ΔtΔ[O2]/Δt. Express your answer to two significant figures and include the appropriate units. Part B Find Δ[H2O]/ΔtΔ[H2O]/Δt. Express your answer to two significant figures and include the appropriate units. Part C Find Δ[S8]/ΔtΔ[S8]/Δt. Express your answer to two significant figures and include the appropriate units. Part D Find the rate of the reaction. Express...
Consider the reaction: 8H2S(g) + 4O2(g) à 8H2O(g) + S8(g) Complete the table including units, Show your work below. ∆[?)?]/∆? ∆[?)]/∆? ∆[?)?]/∆? ∆[?.]/∆? Rate -0.080 M/s
2) Consider the reaction: 8H2S(g) + 402(g) → 8H2O(g) + S8(g) Complete the table including units, Show your work below. A[H2S]/At A[02]/At A[H20]/At A[S2]/At Rate -0.080 M/S
Consider the reaction 8H2S(g)+4O2(g)→8H2O(g)+S8(g) Δ[H2S]/Δt = -0.067 M/s You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. Part A Find Δ[O2]/Δt. Express your answer to two significant figures and include the appropriate units. Δ[O2]/Δt = StartFraction Upper M Over s EndFraction Previous AnswersRequest Answer Incorrect; Try Again; One attempt remaining Part BPart complete Find Δ[H2O]/Δt. Express your answer to two significant figures and include the appropriate units. Δ[H2O]/Δt = 6.7×10−2 Ms Previous Answers Correct...
10. Using the table of standard formation enthalpies that you will find below, calculate the reaction enthalpy of this reaction under standard conditions: 8H2S(g)+ 402(g) Ss(s) + 8H2O(0) Round your answer to the nearest kJ. reactant or product H2S(g Ss(s) Standard formation rection -206 H(+ 8SH2Sg) 0 0 H2O)
H2S (g) ---------> 1/8 S8 (s) + H2 (g) delta H rxn = +20.2 kJ What is delta H when 25.00g of S8 reacts? Is correct answer +1.97kJ or +15.7kJ? Could you please explain your answer for me?
Consider the reaction Cl_2(g) + 3F_2(g) rightarrow 2CIF _3 (g) Delta [Cl_2]/Delta t = -0.077 M/s Find Delta [F_2]/Delta t Express your answer to two significant figures and include the appropriate units. Find Delta [CIF_3]/Delta t Express your answer to two signific ant figures and include the appropriate units.
please explain well. I don't understand at all. Explain all steps ans math involved. 3. Elemental sulfur is a molecular solid. The most stable allotrope of elemental sulfur is actually the eight-membered ring, Ss. Thus, the elemental sulfur in the H2S formation reaction shown in question 1 should actually be written as Sa(s). Use the equilibrium constant given in question 1 to find K for the following reaction: 8H2(g) + S«(s) - 8H2S(8) K ? 1. Ammonia and hydrogen sulfide...
Given the thermochemical reaction below: 2 M2S (s) + 2 H2O (l) -> 2M(s) + 2 H2S(g) + O2(g) Delta H* = 595.6 kJ. Where M is a metal and M(s) is the reference form of metal. The Delta H*f of M2S is?
For the reaction H2(g) + S(s) --> H2S(g) delta H = -20.2 kJ mol-1 and delta S =+43.1 J K-1mol-1. Which of the following statements is true? The reaction is spontaneous at all temperatures. delta G becomes less favorable as T is raised. The reaction is only spontaneous at high temps. The reaction is only spontaneous at low temps. The reaction is at equilibrium at 25 C under standardconditions. Please explain why too. Thank you, feedback will beawarded as soon...