The value of KC for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 × 10-4 at 1400 K. 2H2S(g)<---> 2H2(g) + S2(g)
A sample of gas in which [H2S] = 5.40 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.
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The value of KC for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 ×...
The value of KC for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 × 10-4 at 1400 K. 2 H2S (reversible) 2 H2 + S2 A sample of gas in which [H2S] = 5.25 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.
The value of Kc for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 x 104 at 1400 K. 2H,S(g) 2H2(g) +S2(g) 3rd attempt Feedback Inul See Periodic Table See Hint A sample of gas in which (H2S] -4.25 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H,S]? Assume no H2 or Sy was present in the original sample. M
The value of Kc for the thermal decomposition of hydrogen sulfide, shown below, is 2.2x 104 at 1400 K 2H,s(g)-2H2(g) +S2(g) 2nd attempt See Periodic Table SeeHint A sample of gas in which H2S = 3.85 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.
@ See page 648 14 Question (1 point) The value of Kc for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 x 10-4 at 1400 K. 2H,S(g) + 2H2(g) + S2 (8) v 1st attempt . See Periodic Table D See Hint A sample of gas in which [ HS] = 5.40 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or...
@ See page 648 14 Question (1 point) The value of Kc for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 x 10-4 at 1400 K. 2H,$(g) + 2H2(g) +S2(g) V 3rd attempt See Periodic Table D See Hint A sample of gas in which [H2S] = 3.00 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in...
PLEASE HELP WITH THESE QUESTIONS, THANK YOU IN ADVANCE. ********************* The value of Kcfor the thermal decomposition of hydrogen sulfide, shown below, is 2.2 x 104 at 1400 K. 2H2S(g)2H2(g) 4th attempt 晶See PeriodicTable See Hint A sample of gas in which [H2S -4.85 M is heated to 1400K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.
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 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 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
Equilibrium constant A flask is filled with 1.0 M hydrogen sulfide gas and allowed to react according the balanced chemical equation: 2H2S(g) -------- 2H2(g) +S2(g). At equilibrium, [S2] = 0.36 M. Calculate the value of Kc for this reaction. It may help to use a table.