Part A
Calculate KP at 298 K for the reaction NO(g)+12O2(g)→NO2(g) assuming that ΔH∘R is constant over the interval 298-600 K.
Part B
Calculate KP at 480. K for this reaction assuming that ΔH∘R is constant over the interval 298-600
Part C
Do you expect KP to increase or decrease as the temperature is increased to 600. K?
a) to increase |
b)to decrease |
Part A Calculate KP at 298 K for the reaction NO(g)+12O2(g)→NO2(g) assuming that ΔH∘R is constant...
Calculate KP at 499 K for the reaction NO(g) + 1/2O2(g) → NO2(g) assuming that ΔH°R is constant over the interval 298-600 K.
1 2 Part A Calculate Kp at 298 K for the reaction NO(g) + + O2(g) → NO2 (g) assuming that AH is constant over the interval 298-600 K. Kp = 2.31x106 Submit Previous Answers ✓ Correct Part B Calculate Kp at 477 K for this reaction assuming that AHR is constant over the interval 298-600 K. PO AQ * o o ? Kp = | Submit Previous Answers Request Answer Revie For the reaction 2CH4 (g) = C2H2(g) +...
Calculate ΔG∘R at 594 K assuming that ΔH∘R is constant in the temperature interval of interest. Part A Calculate ΔGe for the reaction Express your answer to four significant figures and include the appropriate units. CO(g) + ,02 (g) CO2 (g) at 298.15 K ΔGR: -2572x105 J-mol 1 Previous Answers Correct Part B Calculate ΔGk at 594 K assuming that ΔΗ¡ is constant in the temperature interval of interest Express your answer to four significant figures and include the appropriate...
The equilibrium constant, Kp, for the following reaction is 6.25 at 298 K. 2NO(g) + Br2(g) 2NOBr(g) If ΔH° for this reaction is -16.1 kJ, what is the value of Kp at 187 K? Kp =
The equilibrium constant, Kp, for the following reaction is 0.160 at 298 K. Calculate K, for this reaction at this temperature. 2NOBr(g) 2NO(g) + Br2(g) Kc =
10a 10b. The equilibrium constant, Kp for the following reaction is 0.110 at 298 K. Calculate Kc for this reaction at this temperature. NH4HS(s) NH3+ H2S(g) Ko The equilibrium constant, Kc, for the following reaction is 5.10x10-6 at 548 K. Calculate Kp for this reaction at this temperature NH4CI(sNH)+ HCI(g) Kp
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) NH3(g) + H2S(g) If ΔH° for this reaction is 92.7 kJ, what is the value of Kp at 212 K? Kp =
The reaction below has an equilibrium constant of Kp=2.26×104 at 298 K. CO(g)+2H2(g)⇌CH3OH(g) Part A Calculate Kp for the reaction below. CH3OH(g) CO(g)+2H2(g) Submit My Answers Give Up Part B Reactants will be favored at equilibrium. O Products will be favored at equilibrium. Submit My Answers Give Up Part C Calculate Kp for the reaction below. 를 CO (g) + H2 (g)- CH, OH (g) K=
Calculate Kp at 298 K for the reaction SO.(g) + NO2()SO3(g)+NO() SO2(g) SO3(g) NO(g) NO2(g) -300.4 k/mol -370.4 kJ/mol 86.7 kJ/mol 51.8 kJ/mol For the reaction 2NO(g)+02(g)- 2NO2( f iniially P(NO)1.5 atm, PO2)-1.4 atm, and P(NOJ-2.0 atrn, calculate Δ@for this reaction at 25°C. The following data is valid at 25°C: NO NO2 AGe(kJ/mol 86.7 51.8
The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) <----> (arrows both ways) NH3(g) + H2S(g) If ΔH° for this reaction is 92.7 kJ, what is the value of Kp at 391 K? Kp =_______