Consider the following reaction:             2HF(g) ⟷H2(g) + F2(g) (K = 1.00 x10-2) Given 1.00 mole of HF(g), 0.500 mole of H2(g), and 0.750 mole of F2(g) are mixed in a 5.00-L flask, determine the reaction quotient, Q, and the net direction to achieve equilibrium.

A student ran the following reaction in the laboratory at 696 K: 2HI(g) H2(g) + I2(g) When he introduced HI(g) at a pressure of 3.40 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of HI(g) to be 2.68 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp =

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

The equilibrium constant for the following reaction is 67.6 at 232 °C. PCI 3(g) + Cl₂(g) PCI5(g) K = 67.6 at 232 °C Calculate the equilibrium constant for the following reactions at 232 °C. (a) PCI5(g) PCl3(g) + Cl₂(g) K= (b) 2 PCI5(g) 2 PCI3(g) + 2 Cl₂(g) K=

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Some CH,Cl, is placed in a sealed flask and heated to 589 K. When equilibrium is reached, the flask is found to contain CH,Cl2 (4.80×102 M), CH4 (4.04x10 2 M), and CCl, (4.36x102 M). What is the value of the equilibrium constant for this reaction at 589 K? 2CH;Cl½(g)= CHĄ(g)+ CC14(g) K=

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 5.0 L flask with 4.5 atm of ammonia gas and 4.5 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 2.0 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 = | olo x10 Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility .......................................

Consider the formation of phosgene: CO(g) + Cl₂(g) = COCl₂(g) Into a sealed 1.50 L flask, chemist placed 3.00 × 10-² mol of phosgene gas (COCl₂) and heated it to 800.0 K. After the system reached equilibrium, the pressure of CO was found to be 0.504 bar. Calculate the equilibrium constant Kp for this reaction. Calculate the initial pressure (in bar) of the phosgene gas. R = 0.08314 L.bar/mol K.