A student ran the following reaction in the laboratory at 695 K: N2(g) + 3H2(g) 2NH3(g) When she introduced 4.09x10-2 moles of N2(g) and 7.14x10-2 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3(g) to be 1. 99x10-3 M

A chemical engineer is studying the following reaction: HCH3CO2(aq)+CH3NH2(aq) → CH3CO2(aq) + CH3NH3(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.54. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound concentration expected change in concentration HCH,CO₂ 1.01 M O↑ increase CH3NH2 1.22 M O decrease O↑ increase O decrease O (no change) O (no change) A CH,CO, 0.64 M O↑ increase O decrease O (no change) CH, NH3 1.04 M O ↑ increase O decrease O (no change) HCH CO₂ 0.33 M O↑ increase O decrease O(no change) CHÍNH, 0.50 M O↑ increase O decrease O (no change) B CH,CO, 1.01 M O increase O decrease O (no…

A student ran the following reaction in the laboratory at 675 K: H2(g) + I2(g) 2HI(g) When she introduced 0.226 moles of H2(g) and 0.248 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.11×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =

Part A For the reaction 3H2 (g) + N2 (g) = 2NH3 (g) at 225 °C the equilibrium contant is 1.7 × 102. If the equilibrium mixture contains 0.13 M H2 and 0.018 M N2 , what is the molar concentration of NH3 ? Express your answer to two significant figures and include the appropriate units.

A student ran the following reaction in the laboratory at 1101 K:2SO2(g) + O2(g)      2SO3(g)When she introduced 0.104 moles of SO2(g) and 0.101 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 7.28×10-2 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.

A student ran the following reaction in the laboratory at 543 K: CoCl₂(g) CO(g) + Cl₂(g) When she introduced 1.10 moles of COCI₂(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.94-102 M. Calculate the equilibrium constant, K, she obtained for this reaction.

Nitric acid and nitrogen monoxide react to form nitrogen dioxide and water, like this: 2 HNO3(aq)+NO(9)→3 NO2(g)+H,0(1) At a certain temperature, a chemist finds that a 4.0 L reaction vessel containing a mixture of nitric acid, nitrogen monoxide, nitrogen dioxide, and water at equilibrium has the following composition: compound amount HNO3 5.2 g NO 19.8 g NO, 7.9 g H,O 134.3 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. °C K_ = 0 x10 C

The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K.NH4Cl(s) NH3(g) + HCl(g)Calculate the equilibrium concentration of HCl when 0.227 moles of NH4Cl(s) are introduced into a 1.00 L vessel at 548 K.[HCl] =  M

A student ran the following reaction in the laboratory at 735 K: N2(g) + 3H2(g) = 2NH3(g) When she introduced 0.0402 moles of N2 (g) and 0.0547 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3 (g) to be 0.000861 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Кс =