Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A...
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A 0.500 L reaction vessel initially contains 0.125 mol of H2S and 0.188 mol of H2 at 800∘C. Find the equilibrium concentration of [S2]. Can you please show the math because that's the part that I am struggling with. Thank you!
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Consider the reaction for the decomposition of hydrogen
disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A...
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A...
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A 0.500 L reaction vessel initially contains 0.175 mol of H2S and 6.25×10−2 mol of H2 at 800∘C. Find the equilibrium concentration of [S2].
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g) Kc = 1.67×10^-7 at 800∘C The...
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g) Kc = 1.67×10^-7 at 800∘C The reaction is carried out at the same temperature with the following initial concentrations: [H2S]=1.00×10^−4M [H2]=0.00M [S2]=0.00M Part A Find the equilibrium concentration of S2
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10-7 at 800∘C The...
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10-7 at 800∘C The reaction is carried out at the same temperature with the following initial concentrations: [H2S]=3.20×10-4M [H2]=0.00M [S2]=0.00M Find the equilibrium concentration of S2. Express the concentration to three significant figures and include the appropriate units.
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) = 2H2(g) + S2(g), Kc =...
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) = 2H2(g) + S2(g), Kc = 1.67 x 10-7 at 800°C The reaction is carried out at the same temperature with the following initial concentrations: [H2S] [H2] [S2] 4.00 x 10-4M 0.00 M 0.00 M - Part A Find the equilibrium concentration of S2. Express the concentration to three significant figures and include the appropriate units. HA ? [S2] = Value Units
find the equilibruim constant of S2. please show steps Consider the reaction for the decomposition of...
find the equilibruim constant of S2. please show steps
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) = 2H2(g) + S2(g), Kc = 1.67 x 10-7 at 800°C A 0.500 L reaction vessel initially contains 0.200 mol of H2S and 6.25x10-2 mol of H2 at 800°C.
The following reaction 2H2S(g)⇌2H2(g)+S2(g),Kc=1.67×10−7 at 800∘C2H2S(g)⇌2H2(g)+S2(g),Kc=1.67×10−7 at 800∘C is carried out at 800 ∘C∘C with the...
The following reaction 2H2S(g)⇌2H2(g)+S2(g),Kc=1.67×10−7 at 800∘C2H2S(g)⇌2H2(g)+S2(g),Kc=1.67×10−7 at 800∘C is carried out at 800 ∘C∘C with the following initial concentrations: [H2S]=0.100M[H2S]=0.100M, [H2]=0.100M[H2]=0.100M, and [S2]=0.00 M[S2]=0.00 M. Find the equilibrium concentration of S2S2. Express the molarity to three significant figures. [S2]eq[S2]eq = nothing MM
1. Consider the reaction for the decomposition of hydrogen disulfide: H2S(g) = 2H2(g) + S2(g) With...
1. Consider the reaction for the decomposition of hydrogen disulfide: H2S(g) = 2H2(g) + S2(g) With an equilibrium constant of 1.67x10-7 (at 800 °C). If a 0.500 L reaction vessel initially contains 0.0125 moles of H2S. Find the equilibrium concentrations of the products; H2 and S2. (25 points)
The reaction 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7, at 800∘C is carried out with the following initial concentrations: [H2S] =...
The reaction 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7, at 800∘C is carried out with the following initial concentrations: [H2S] = 0.375 M , [H2] =0.125 M , and [S2] = 0.000 M. Find the equilibrium [S2]. Express your answer with the appropriate units.
The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] =...
The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] = 0.275 M , [H2] =0.300 M , and [S2] = 0.00 M. Find the equilibrium concentration of [S2].
The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] =...
The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] = 0.175 M , [H2] =0.350 M , and [S2] = 0.00 M. Find the equilibrium concentration of [S2].
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) = 2H2(g) + S2(g), Kc = 1.67 x 10-7 at 800°C The reaction is carried out at the same temperature with the following initial concentrations: [H2S] [H2] [S2] 4.00 x 10-4M 0.00 M 0.00 M - Part A Find the equilibrium concentration of S2. Express the concentration to three significant figures and include the appropriate units. HA ? [S2] = Value Units
find the equilibruim constant of S2. please show steps
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) = 2H2(g) + S2(g), Kc = 1.67 x 10-7 at 800°C A 0.500 L reaction vessel initially contains 0.200 mol of H2S and 6.25x10-2 mol of H2 at 800°C.
1. Consider the reaction for the decomposition of hydrogen disulfide: H2S(g) = 2H2(g) + S2(g) With an equilibrium constant of 1.67x10-7 (at 800 °C). If a 0.500 L reaction vessel initially contains 0.0125 moles of H2S. Find the equilibrium concentrations of the products; H2 and S2. (25 points)
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