For the reaction X(g) + 2Y(g) = 3Z(g) Kp = 2.08x10-2 at a temperature of 325 °C . Calculate the value of Kc . Express your answer numerically. • View Available Hint(s) ΑΣφ ? Ke %3D
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Given reaction:
Given, Kp = at
We have to find the value of Kc.
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- Estimate the value of the equilibrium constant at 525 K for following reaction a) 2CO(g) + O2(g) (Equilibrium arrows) 2CO2(g) CO(g) O2(g) CO2(g) Delta H standard (kj/mol) -110.5 0 -393.5 Delta G standard (kj/mol) -137.2 0 -394.4 Delta S standard (j/mol time k) 197.7 205.2 213.8Find ∆H as a function of T for the reaction: CO2 (g) + C (s, graphite) = CO Given that ∆H 293= 41,400 cal Cp CO2= 5.166+15.77×10^-3 T - 95.78×10^-3 T² + 2.260×10^-9 T³ Cp CO= 6.6 + 2×10^-3 T Cp C (s, graphite)= 2.673 + 2.617×10^-3 T - 1.169×10^-5 T^-2A student conducted an experiment to determine the Ksp of Ca(OH)2 at T = 298 K. The value he calculated was 5.4 x 10-6 and when he looked the theoretical value, he found that it is 5.1 x 10-6. Give the possible sources of error why the calculated value was higher than the theoretical value
- Estimate the difference between ΔHreaction and ΔUreaction (in kJ/mol) for the reaction: 6Li(s) + N2(g) →2Li3N(s) at 298 KCO(g)+2H2(g)⇌CH3OH(g) K = 2.18×102 at 340 K Calculate ΔrG for the reaction at 340 K in STANDARD CONDITIONS please Express your answer using three significant figures and include the appropriate units.Determine the equilibrium constant for the reaction below using the following information: 2 JQ ⇌ J2 + Q2 KC = 0.28 3.5 J2 + 3.5 Q2 ⇌ 7 JQ KC = ? Group of answer choices -0.98 171 13 -0.012 86
- At what temperature will the transformation: Cu(s) ⇌ Cu(g) occur spontaneously if ∆H° = 342.0 kJ/mole and ∆S° = 146.2 J/mole KFor boiling of propyl alcohol (CH3 CH2 CH2 OH), the reactionCH3 CH2 CH2 OH ---> CH3 CH2 CH2 OH(g)it is found that Hrxn = 47.5 kJ/mol and Srxn = 129.0 J/molK. a) Based on the above data, estimate the value for Tb, the normal boiling point for propyl alcohol. b) The experimental value for the normal boiling point for propyl alcohol is Tb = 97. C. Is this the same (to within +-1. C) as the value found in part a? If not, explain why the value in part a is different than the experimental value?For the reaction A (g) → 2 B (g), K = 14.7 at 298 K. What is the value of Q for this reaction at 298 K when ∆G = -19.3 kJ/mol?
- For the reaction A + B <=> AB, kassoc = 2.0 sec-1 M-1 and kdissoc = 0.5 sec-1. This means that Kassoc is equal to ____ M-1. (Enter your answer to the nearest 0.1; do not include units)Consider the following reaction. 2 SO2(g) + 02(g) ---> 2 SO3(g) What is the relationship between the reaction quotient (Q) and the equilibrium constant (Kc) for this reaction at the moment excess 02(g) is added? Group of answer choices Q > Kc No answer text provided. Q < Kc Q = KcFor the reaction: N2O4(g) ↔ 2NO2 (g)Between 298 and 900 K, it is true that: Kp = αTbe-c / T(a) Deduce expressions for ∆Gr°, ∆rH° and ∆rS° as a function of temperature, for this reaction.(b) Calculate ∆Gr°, ∆rH° and ∆rS° for the reaction at 600 K, knowing that α = 1.09x1013; b = -1.304 and c = 7307