Consder the following equilibrum  PCl3 (g) + Cl2 (g) ↔ PCl5 (g) ΔrH°=-92 kJ/mol The concentration of PCl3 at equilibrium may be increased by     adding a catalyst     increasing the pressure through decreasing the volume     adding PCl5 to the system     decreasing the temperature     adding Cl2 to the system

Consider the following equilibrium: Cl2(3) + F2(3) = 2CIF(g) with Keg = 19.9 If we begin with O.100 atm chlorine and 0.100 atm fluorine, what are the partial pressures of CIF and F2 at equilibrium? O 0.20 atm, 0.0 atm O 19.9 atm, 0.00 atm 0.138 atm, 0.031 atm 0.182 atm, 0.009 atm O 0.10 atm, 0.050 atm

Which of the following change will shift the equilibrium to the right for the following reaction?                 CaCO3(s) ------> CaO(s) + CO2(g) Group of answer choices Increasing CaCO3(s) Decreasing the pressure Decrease CaO(s) Increasing CO2 (g)

For the equilibrium system below, which of the following would result in an increase in the quantity of PC15(g)? PC13(g) + Cl₂(g) PC15(g) + 45 kJ increasing temperature decreasing temperature removing some Cl2(g) increasing the size of the container injecting some He gas

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H2(g) + Consider the following equilibrium mixture in a closed system: H2O(g) + CO(g) CO2(g). Explain what would happen to the equilibrium upon the addition of hydrogen gas? ○ The addition of hydrogen gas would not disrupt the equilibrium, so nothing would happen The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the right which would result in more CO2 being produced until equilibrium is achieve ○ The addition of hydrogen gas would disrupt the equilibrium causing it to shift towards the left which would result in more reactants being produced until equilibrium is achieved

Carbon dioxide and water react to form methanol and oxygen, like this: 2 CO,(g)+4 H,O(g)→2 CH;OH(1)+3 O,(g) At a certain temperature, a chemist finds that a 4.6 L reaction vessel containing a mixture of carbon dioxide, water, methanol, and oxygen at equilibrium has the following composition: compound amount CO2 3.94 g H,0 4.50 g CH,OH 3.68 g O2 2.67 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. M K = 0 Lo B Cisc M Explanation Check A Chem 02022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility 9 Type here to search (99+ IA ASUS ZenBook Esc F2 F3 F4 F5 F6 F7 F8 %23 %24 21 4. * 6. L. R Y 3)

If you decrease the volume of a system containing the following reaction at equilibrium, identify which way will the equilibrium will shift and explain why? 2NO(g) + Cl 2 (g) ↔ 2NOCl(g)

Mercury(II) oxide decomposes to form mercury and oxygen, like this: 2 HgO(s)→2 Hg(1)+O2(g) At a certain temperature, a chemist finds that a 3.3 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the following composition: compound amount HgO 19.5 g Hg 14.6 g O2 0, 17.4 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 x10

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature.  If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?