The equilibrium concentration of H2 is 1.702 * 10-3 M
Saved 1 attempts left Check my work Enter your answer in the provided box. Hydrogen sulfide...
Enter your answer in the provided box. 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 0.35 mol of H2S is placed in a 3.0−L container, what is the equilibrium concentration of H2(g) at 700°C?
Enter your answer in the provided box. 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 0.43 mol of H2S is placed in a 3.0−L container, what is the equilibrium concentration of H2(g) at 700°C?
Enter your answer in the provided box. Hydrogen sulfide decomposes according to the following reaction, for which K.-9.30 x 10-8 at 700°C: 2 H,S(g) = 2 H2(g) +S2() If 0.41 mol of H2S is placed in a 3.0-L container, what is the equilibrium concentration of H2(g) at 700°C?
Enter your answer in the provided box. 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 0.41 mol of H2S is placed in a 3.0L container, what is the equilibrium concentration of H2(g) at 700°C?
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
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
Hydrogen sulfide decomposes according to the following reaction, for which Kc = 9,30 x 10^-8 at 700 degree C.2 H2S(g)leftrightharpoons 2H2(g) + S2(g)It 0.42 mol H2S is placed in a 2.8 L container, what is the equilibrium concentration of H2(g) at 700 degree C? 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
1 attempts left Check my work Enter your answer in the provided box. Ammonia (NH3) decomposes to hydrogen and nitrogen and 22.0 kcal/mol of energy is absorbed. 2 NHj(g) 3 H2(8) + N2(g) AH +22.0 kcal/mol How much energy is absorbed when 2.63 g of NHj reacts? keal of energy absorbed Report your answer to appropriate number of significant figures.