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The balance between SO2 and SO3 is important in understanding acid rain formation in the troposphere. From the following information at 25°C
calculate the equilibrium constant for the reaction
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Chapter 20 Solutions
Chemistry
- 2A(g) = B(g) + 2C(g)At 100C, 1.61 mol of A were placed in a 5.00 L container and the reaction was allowed to proceed. After equilibrium was established, it was found that 70.4% of A had decomposed. What is the value of Kc for this reaction at 100C?arrow_forward1.25 moles of NOClwere placed in a 2.50 L reaction chamber at 427ºC. After equilibrium was reached, 1.10 moles of NOCl remained. Calculate the equilibrium constant, Kc, for the reaction 2NOCl(g) -> 2NO(g) + Cl2(g).arrow_forwardConsider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g) 6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?arrow_forward
- 9.Suppose 1.000 mole of CO and 3.000 mol of Hydrogen are put in a 10.000 L vessel at 1200 K. Determine the equilibrium composition of the reaction mixture if K. = 3.92 for the reaction. CO (g) + 3H₂(g) → CH4(g) + H₂O(g)arrow_forwardNitrogen monoxide and hydrogen react to form nitrogen and water, like this: 2 NO(9)+2H,(9)→ N2(9)+2H,O(9) Write the pressure equilibrium constant expression for this reaction.arrow_forwardPhosphorus tribromide decomposes to form phosphorus and bromine, like this: 4 PBr,(9)→P(9)+6 Br,(g) Write the pressure equilibrium constant expression for this reaction. ?arrow_forward
- Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 500. mL flask with 3.4 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.4 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K, = 0 Ox10arrow_forwardThe equilibrium constants (expressed in atm) for the chemical reaction N2(g) + O2(g) ⟷⟷ 2NO(g) are KP = 1.1 × 10–3 and 3.6 × 10–3 at 2200 K and 2500 K, respectively. Which statement is true? Group of answer choices the total pressure at 2200 K is the same as at 2500 K. the reaction is exothermic, ΔHº < 0. Kp is less than Kc by a factor of (RT). higher total pressure shifts the equilibrium to the left. the partial pressure of NO(g) is less at 2200 K than at 2500 K.arrow_forwardThe equilibrium constant for the reaction, 3 H2(g) + N2(g)= 2NH3(g), at a given temperature is 1.4 x 10–7. Calculate the equilibrium concentration of ammonia, if [H2] = 1.2 x 10–2 mol L–1 and [N2] = 3.2 x 10–3 mol L–1.arrow_forward
- The equilibrium constant, K, for the synthesis of ammonia 6.8 x 105 at 298 K. Predict the value at 400 K The reaction is N2(g) = 3H2(g) ჻ 2NH (g).arrow_forwardFor the hypothetical reaction 2A(g) + B(g) ⇌ 3C(g) + heat, the equilibrium constant is 0.138 at 45∞C. What is the equilibrium constant for reaction, 3C(g) + heat ⇌ 2A(g) + B(g)?arrow_forwardAmmonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200. mL flask with 2.5atm of ammonia gas, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 0.38atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to significant digits.arrow_forward
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning