3NO(g) → N2O(g) + NO2(g)

Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 1.5 L flask with 1.7 atm of ammonia gas and 2.1 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 0.77 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = ☐ P x10

Calculating an equilibrium constant from a partial equilibrium composition

O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 1.9 mol of NO,, 0.10 mol of N0 and 1.7 mol of CO,. The following reaction becomes possible: 2' NO,(g)+CO(g) -NO(g)+CO,(g The equilibrium constant K for this reaction is 4.70 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M TRADIS Explanation Check 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy | Acces NOV 242 PAGES étv 4 MacBook Air II

What does it mean for a chemical reaction to reach equilibrium?         The rates of the forward and reverse reactions are equal. The concentrations of the reactants and products are also equal.         The rates of the forward and reverse reactions are increasing. The concentrations of the reactants and products are equal.         The rates of the forward and reverse reactions are equal. The concentrations of the reactants and products are constant.         The rates of the forward and reverse reactions are increasing. The concentrations of the reactants and products are also increasing.

Write balanced net ionic equations for the following reversible reactions. Then write the corresponding equilibrium constant, k, for each. 1) Hydrogen gas reacts with nitrogen has to form ammonia gas and steam. 2) Nitrogen gas reacts with solid sodium carbonate and solid carbon to produce carbon monoxide gas and solid sodium cyanide (NaCN).

Calculating an equilibrium constant from a partial equilibrium composition Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 2.0 L flask with 1.2 atm of ammonia gas and 3.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.3 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = [] P x10 X ? olo 18 Ar 8.