1 H2S(g) 2 H2(g) + S2(g)
Kp= 9.30x10-8 at 70 degrees celcius. If 0.45 mol of H2S is placed in a 3.00 L container, what is the equilibrium concentration of H2(g) at 700 degrees celcius?
1 H2S(g) 2 H2(g) + S2(g) Kp= 9.30x10-8 at 70 degrees celcius. If 0.45 mol of H2S...
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?
Hydrogen sulfide decomposes according to the following reaction, for which Kc=9.30x10^-8 at 700 degrees C: 2 H2S(g)<-------> 2 H2(g) + S2(g) If 0.57 mol of H2S is placed in 3.0-L container, what is the equlilibrium concentration of H2(g) at 700 degrees C? _______ M
6. If 0.54 mol of H2S is placed in a 3.0 L container, what is the equilibrium concentration of H2 at 710 C? 6. In the decomposition of hydrogen sulfide: 2H2S(9) + 2H2(g) + S2(g) K = 9.90 x 10-8 at 710°C If 0.54 mol H2S is placed in a 3.0 liter container, what is the equilibrium concentration of H2(g) at 710 °C? Can the small x approximation be used here? Justify it (see p. 768 of text). (1.9 x...
At a certain temperature, the Kp for the decompositon of H2S is 0.834. H2S(g) <---> H2(g) + S(g) Initally, only H2S is present at a pressure of 0.108 bar in a closed container. What is the total pressure in the container at equilibrium?
At a certain temperature, the Kp for the decomposition of H2S is 0.800. H2S(g) H2(g) + S(g) Initially, only H2S is present at a pressure of 0.236 atm in a closed container. What is the total pressure in the container at equilibrium?
Hydrogen sulfide decomposes according to the following reaction, for whichKc = 9.30 × 10−8 at 700°C: 2 H2S(g) ⇌ 2 H2(g) + S2(g) If 0.27 mol of H2S is placed in a 3.0−L container, what is the equilibrium concentration of H2(g) at 700°C? ____M
2 H2S(g) ⇌ 2 H2(g) + S2(g) Kc = 9.0 × 10−8 at 700°C the initial concentrations of the three gases are 0.500 M H2S, 0.500 M H2, and 0.250 M S2. Determine the equilibrium concentrations of the gases.
A mixture of 0.01341 mol of CH4, 0.01170 mol of H2S, 0.02118 mol of CS2, and 0.02835 mol of H2 is placed in a 1.0-L steel pressure vessel at 3416 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g) 1 CS2(g) + 4 H2(g) At equilibrium 0.003198 mol of H2S is found in the reaction mixture. - Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2. - Calculate KP for this reaction.
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
At a certain temperature, the Kp for the decomposition of H2S is 0.719. H2S(g)=H2(g)+S(g) Initially, only H2S is present at a pressure of 0.277 atm in a closed container. What is the total pressure in the container at equilibrium?