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 ×...
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.
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,$(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...
@ 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...
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 sulfide: 2 H2S(g) ⇌ 2 H2(g) + S2(g) A 0.300 L vessel initially contains 0.450 mol of H2S at 800oC. Find the equilibrium concentration of S2. Kc = 1.67 x 10-7 at 800oC. 1) 3.54 × 10-4 M 2) 0.00204 M 3) 0.00455 M 4) 1.94 × 10-4 M 5) 0.00551 M
Hydrogen sulfide decomposes according to the following equation, for which Kc = 0.0000728 at a given temperature. 2 H2S(g) <=> 2 H2(g) + S2(g) If 7.37mol of H2S is placed in a 3.0 L container, what is the equilibrium concentration of H2(g)? Give your answer to 3 decimal places
Hydrogen sulfide decomposes according to the following reaction, for which Kc = 9.30 × 10−8 at 700°C: 2 H2S(g) ⇌ 2 H2(g) + S2(g) If 0.55 mol of H2S is placed in a 3.0−L container, what is the equilibrium concentration of H2(g) at 70 degrees Celcius?
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].