Question

In: Chemistry

8H2S(g)+4O2(g)→8H2O(g)+S8(g) Δ[H2S]/Δt = -0.012 M/s a)Find Δ[O2]/Δt. b)Find Δ[H2O]/Δt. c)Find Δ[S8]/Δt. d)Find the rate of the...

8H2S(g)+4O2(g)→8H2O(g)+S8(g) Δ[H2S]/Δt = -0.012 M/s

a)Find Δ[O2]/Δt.

b)Find Δ[H2O]/Δt.

c)Find Δ[S8]/Δt.

d)Find the rate of the reaction.

Expert Solution

rate = decrease in concentration of reactant / time taken = increase in concentration of product / time taken.

a)

-1/8 [H2S] / t = -1/4 [O2] / t

[H2S] / t = - 0.012 M/s

[O2] / t = 4/8 [H2S] / t

[O2] / t = 4/8 (-0.012 )

[O2] / t = - 0.006 M/s

b)

-1/8 [H2S] / t = 1/8 [H2O]/t

- [H2S] / t = [H2O]/t

[H2O]/t = - (0.012)

[H2O]/t = 0.012 M/s

c)

1/8 [H2O]/t = [S8] / t

[S8] / t = 1/8 (0.012)

[S8] / t = 0.0015 M/s

d)

rate = [S8] / t

rate = 0.0015 M/s

queen_honey_blossom answered 7 months ago

Consider the reaction: 8H2S(g)+4O2(g)→8H2O(g)+S8(g) Δ[H2S]/Δt = -0.087 M/s 1) Find Δ[O2]/Δt 2) Find Δ[H2O]/Δt 3) Find...

Consider the reaction: 8H2S(g)+4O2(g)→8H2O(g)+S8(g) Δ[H2S]/Δt = -0.087 M/s 1) Find Δ[O2]/Δt 2) Find Δ[H2O]/Δt 3) Find Δ[S8]/Δt 4) Find the rate of the reaction.

1 If Δ[BrO3- ]/Δt = 0.037 M/s. What is [BrO- ]/Δt in M/s? 2 The rate...

1 If Δ[BrO3- ]/Δt = 0.037 M/s. What is [BrO- ]/Δt in M/s? 2 The rate of change of [B] is -0.301 M/min. What is the rate of reaction for the following reaction in M/min? 2A + 5B → 3C + 7D 3 Under a different set of conditions, the rate of change of [C] is 0.194 M/min. What is the rate of change of [D] in M/min? 4 If the rate of change of [C] is 0.038 M/min. What...

Consider the reaction: 8H2S(g)+4O2(g)?8H2O(g)+S8(g) ?[H2S]/?t = -0.047M/s . Find ?[O2]/?t Express your answer to two significant...

Consider the reaction: 8H2S(g)+4O2(g)?8H2O(g)+S8(g) ?[H2S]/?t = -0.047M/s . Find ?[O2]/?t Express your answer to two significant figures and include the appropriate units Find ?[H2O]/?t Express your answer to two significant figures and include the appropriate units. Find ?[S8]/?t Express your answer to two significant figures and include the appropriate units. Find the rate of the reaction. Express your answer to two significant figures and include the appropriate units.

[A], M [B], M Δ [C]/ Δ t (initial) M/s 0.215 0.150

[A], M [B], M Δ [C]/ Δ t (initial) M/s 0.215 0.150 5.81 x 10–4 0.215 0.300 1.16 x 10–3 0.430 0.150 2.32 x 10–3 Given the initial rate data for the reaction A + B ? C, determine the rate expression for the reaction. Please show steps and explain please

If Δ[ClO]/Δt at 298 K is 22.94×10–6 M/s, what is the rate of change in [Cl2]...

If Δ[ClO]/Δt at 298 K is 22.94×10–6 M/s, what is the rate of change in [Cl2] in the following reaction? 2ClO(g)= Cl2(g)+O2(g)

For the reaction A + H2O → products, find the rate of the reaction when [A] = 0.75 M, k= 0.02. a) 0.077 s-1 b) 0.085 s-1 c) 0.015 s-1 d) 0.026 s-1

Balance the following skeleton reaction and identify the oxidizing and reducing agents: H2S(g) +NO3-(aq) --> S8(s)...

Balance the following skeleton reaction and identify the oxidizing and reducing agents: H2S(g) +NO3-(aq) --> S8(s) + NO(g) [acidic]. Include the states for each reactant and product in the balanced chemical equation. Do not include the states when identifying the oxidizing and reducing agents.

Calculate ΔrH for the following reaction: C(s)+H2O(g)→CO(g)+H2(g) Use the following reactions and given ΔrH's. C(s)+O2(g)→CO2(g), ΔrH=...

Calculate ΔrH for the following reaction: C(s)+H2O(g)→CO(g)+H2(g) Use the following reactions and given ΔrH's. C(s)+O2(g)→CO2(g), ΔrH= -393.5 kJmol−1 2CO(g)+O2(g)→2CO2(g), ΔrH= -566.0 kJmol−1 2H2(g)+O2(g)→2H2O(g), ΔrH= -483.6 kJmol−1 Express your answer using one decimal place.

Give the symmetry number for each of the following molecules a)Co b)O2 c)H2S d)SiH4 and e)CHCl3. ...

Give the symmetry number for each of the following molecules a)Co b)O2 c)H2S d)SiH4 and e)CHCl3. Also explain please and include diagram if possible

At 22°C, Kp = 0.070 for the equilibrium: NH4HS (s) NH3 (g) + H2S (g) a)...

At 22°C, Kp = 0.070 for the equilibrium: NH4HS (s) NH3 (g) + H2S (g) a) A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4HS remains. b) After the equilibrium in part a) was established, the reaction flask is then charged with an additional 0.59 atm of NH3. When the system has equilibrated, what is the partial pressure of hydrogen sulfide?