The standard enthalpy of reaction (i.e. ΔH°) for a particular reaction is −20.1 kJ/mol. At 16.0 °C the equilibrium constant for the reaction is 2.30 × 103. Calculate the temperature (in °C) at which the equilibrium constant, K = 8.45 × 104. R = 8.314472 J⋅mol−1⋅K−1. Report your answer to THREE significant figures.
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The standard enthalpy of reaction (i.e. ΔH°) for a particular reaction is −20.1 kJ/mol. At 16.0...
part 1 Calculate the equilibrium constant at 184 °C for a reaction that has a standard enthalpy of reaction, ΔH° = 30.2 kJ/mol and an equilibrium constant, K = 0.0603 at 10.6 °C. R = 8.314472 J⋅mol−1⋅K−1. Report your answer to THREE significant figures. part 2 The standard enthalpy of reaction (i.e. ΔH°) for a particular reaction is −31.7 kJ/mol. At 24.9 °C the equilibrium constant for the reaction is 3.96 × 10−2. Calculate the temperature (in °C) at which...
Calculate the equilibrium constant at 177 °C for a reaction that has a standard enthalpy of reaction, ΔH° = 21.3 kJ/mol and an equilibrium constant, K = 0.0612 at 40.5 °C. R = 8.314472 J⋅mol−1⋅K−1. Report your answer to THREE significant figures.
The energy of activation for a particular reaction is 11.1 kJ/mol. At 18.9 °C the rate constant of the reaction is 1.67 × 102s.-1 Calculate the temperature (in °C) when the rate constant, k = 4.99 × 103s.-1 R = 8.314472 J⋅mol-1⋅K-1. Report your answer to THREE significant figures.
The change in enthalpy (?Horxn) for a reaction is -29.6 kJ/mol . The equilibrium constant for the reaction is 4.3×103 at 298 K. Part A What is the equilibrium constant for the reaction at 686 K ? Express your answer using two significant figures.
1a) Consider the following reaction: 3 C(s) + 4 H2(g) → C3H8(g); ΔH° = –104.7 kJ; ΔS° = –287.4 J/K at 298 K What is the equilibrium constant at 298 K for this reaction? Report answer to TWO significant figures. 1b) Τhe enthalpy of vaporization of ammonia is 23.35 kJ/mol at its boiling point (–33 °C). Calculate the value of ΔSsurr when 1.00 mole of ammonia is vaporized at –33 °C and 1.00 atm. Report answer to THREE significant figures.
Liquid nitrogen has a measured enthalpy of vaporization ( ΔH^o vap) = 2.79 kJ/mol and entropy of vaporization ( Δ S^ovap) = 36.1 J/K mol. Calculate the boiling point of liquid nitrogen, in oC using this information. (Use 273.15 K = 0 oC for the temperature conversion. Report your answer with three significant figures.) Tvap = ????? °C I got 196^oC but it is incorrect.
Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D Use the following data: Substance ΔH∘fΔHf∘ (kJ/mol)kJ/mol) AA -273 BB -417 CC 223 DD -475 Express your answer to three significant figures and include the appropriate units.
M14. For a particular reaction, the enthalpy change is AH° = +100 kJ/mol and the entropy change is AS° = + 100 J/mol K. What is the equilibrium constant at 300 K?
The change in enthalpy (AH) for a reaction is -35.7 kJ/mol. The equilibrium constant for the reaction is 1.4x109 at 298 K Part A What is the equilibrium constant for the reaction at 618 K? Express your answer using two significant figures. ΑΣφ ? K-
1. The rate constant for a particular reaction is 1.15 × 105s-1 at 23.7 °C and is 6.88 × 105s-1 at 63.2 °C. Calculate the energy of activation, EA for the reaction in kJ/mol. R = 8.314472 J⋅mol-1⋅K-1. Report your answer to THREE significant figures. 2. What is the correct expression for the equilibrium constant for the following reaction? 2 A + 3 B ⇌ 5 C + 3 D Kc = [C][D] / [A][B] Kc = [C]5[D]3 / [A]2[B]3...