Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. NO2 is a reddish brown gas while N2O4 is colorless. At high temperatures the red color is strong. At low temperatures the gas has less color. If we represent the equilibrium as, N2O4(g) We can conclude that the reaction is 2 NO2(g) 2 NO2(g) N₂O(g) Brown gas Colorless gas Cannana laminaMama Ca Exothermic Endothermic Neutral More information is needed to answer this question

For the reaction at eqlibrlum: 3Fe(s) - 4H20(g) = Fez04(s) + 4H2(9), removing some of the product, Fe3O4(s), would: Multiple Choice Increase the value of the equilibrium constant, K Decrease the value of the equilibrium constant, K Shift the equilibrium to the right Shift the equilibrium to the left Cause no change

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 100. L tank with 42. mol of sulfur dioxide gas and 5.6 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 9.0 mol. Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K_ = ] x10

(Q106) Consider the decomposition of nitrosyl bromide into nitrogen monoxide and bromide gas, which has an equilibrium constant K. = 6.2 x 105 when the reaction occurs at a certain temperature. If the initial concentration of nitrosyl bromide is 0.832 M, what will be the equilibrium concentration of nitrogen monoxide gas? 2 BRNO (g) 2 NO (g) + Br2 (g)

23) 6.0 moles of pure ammonia gas were injected into a 2.0-L flask and allowed to reach equilibrium according to the equation shown below. If the equilibrium mixture was analyzed and found to contain 2.0 moles of nitrogen gas, calculate the value of the equilibrium constant. 2N H3 (g) → N, (g) + 3H2 (g)

Solid carbon dioxide is also called dry ice. Dry ice is placed in a sealed container. Some CO2 sublimes and the following equilibrium is formed: CO2 (s) = CO2 (g) If the amount of solid CO2 (dry ice) in the container is doubled what would happen? (Hint: Write the equilibrium constant expression.)   Solid carbon dioxide is also called dry ice. Dry ice is placed in a sealed container. Some CO2 sublimes and the following equilibrium is formed: CO2 (s) = CO2 (g) If the amount of solid CO2 (dry ice) in the container is doubled what would happen? (Hint: Write the equilibrium constant expression.)   The amount of CO2 (g) would increase, but not double.  The amount of CO2 (g) would double. The partial pressure of CO2 (g) would increase.  The amount of CO2 (g) would not change.

A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant. A(s) B(g) + C(g) Then, the container volume was doubled and equilibrium was re-established. How many moles of A remain? moles of A: mol

Write equilibrium expressions for: N₂(g) + 3H₂(g) 2NH₂(g) 3 the reaction as written • the reverse reaction the reaction as written with all coefficients in the equation halved

For the reaction 2NO(g) + O2(g) → 2NO2(g) at a certain temperature, the equilibrium concentrations were found to be [NO2] = 5.7 × 10–3 M, [O2]= 1.0 × 10–2 M, and [NO] = 2.0 × 10–3 M. Calculate the value of the equilibrium constant from these data.

Consider the following reaction: 4NH3(g) + 6NO(g) → 6H₂0(g) + 5N₂(g) If the initial concentrations of NH3(g) and NO(g) are 4.0 M, at equilibrium [NO] = 1.0 M, calculate the equilibrium concentration of NH3(g). A) 3.0 M B) 2.0 M C) 5.0 M D) 2.5 M E) 0.50 M