Question
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 -...
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 = nothing nothing Request Answer Part B Find Δ[H2O]/Δt. Express your answer to two significant figures and include the appropriate units. Δ[H2O]/Δt = nothing nothing Request Answer Part C Find Δ[S8]/Δt. Express your answer to two significant figures and include the appropriate units. Δ[S8]/Δt = nothing nothing Request Answer Part D Find the rate of the reaction. Express your answer to two significant figures and include the appropriate units. rate = nothing nothing Request Answer Provide Feedback
Exercise 14.32 - Enhanced - with Feedback 5 of 32 > Review Constants Periodic Table Part A Consider the reaction 8H,S(g) + 40, (8)+8H2O(g) +Ss(E) AH,S]/At = -0.067 M/s You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. Find A(02/At. Express your answer to two significant figures and include the appropriate units. A[0]/A1 = Value Units Submit Request Answer Part B Find A[H0]/A. Express your answer to two significant figures and include the appropriate units. A[H0]/At = Value Units Submit Request Answer
Answers
rate of reaction is given as:
rate = sign * (1/x) * Δ[concentration]/Δtsign is negative for reactant and positive for product
x is stoichiometric coefficient in chemical equation
In terms of H2S:
rate = (-1/8) * Δ[H2S]/Δt
rate = (-1/8) * (-0.067 M/s)
= 8.375*10^-3 M/sa)
In terms of O2,
Rate = (-1/4) * Δ[O2]/Δt
8.375*10^-3 M/s = (-1/4)*Δ[O2]/Δt
Δ[O2]/Δt = 0.0335 M/s
Answer: 0.034 M/sb)
In terms of H2O:
rate = (-1/8) * Δ[H2O]/Δt
8.375*10^-3 M/s = (-1/8) * Δ[H2O]/Δt
Δ[H2O]/Δt = 0.067 M/s
Answer: 0.067 M/s
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