An decrease in temperature increases the reaction rate because temperature affec

Question

An decrease in temperature increases the reaction rate because temperature affects the equilibrium constant of the reaction a smaller fraction of the collisions have the correct orientation of molecules. the activation energy of the reaction will decrease. less collisions will have enough energy to exceed the activation energy. the activation energy of the reaction will increase. The equilibrium constant, K_p, for the reaction H_2(g) + I_2(g) doubleheadarrow 2HI(g) is 10.0 at 450 degree C. A rigid cylinder at that temperature contains 1.00 atm of hydrogen, 1.00 aim iodine, and 10.0 atm of hydrogen iodide. Is the system at equilibrium? Yes No. the forward reaction must proceed to establish equilibrium No. the reverse reaction must proceed to establish equilibrium. Need to know the volume of the container before deciding. Depends on the rates of the forward and reverse reactions. Hydro gen bromide will dissociate into hydrogen and bromine gases. H_2(g) + Br_2(g) doubleheadarrow 2HBr(g) Delta H degree = -68 kJ What effect will a temperature increase of 50 degree C have on this system at equilibrium? Mark all correct answers. The partial pressure of hydrogen bromide will increase. The partial pressure of hydrogen will increase. The partial pressure of hydrogen bromide will decrease. The partial pressure of bromine will increase. The partial pressure of bromine will decrease. What is the expression for Q_c for the following unbalanced chemical reaction? (Balance it first!) H_3O^+(aq) + Cl^-(aq) + MnO_2(s) doubleheadarrow Mn^2+(aq) + H_2O(l) + Cl_2(g) [H_3O^+]^4 [Cl^-]^2 [MnO_2]/[Mn^2+] [H_2O]^6[Cl_2] [Mn^2+] [H_2O]^6[Cl_2]/[H_3O^+]^4 [Cl^-]^2[MnO_2] [H_3O^+]^4 [Cl^-]^2/[Mn^2+] [Cl_2] [Mn^2+] [Cl_2]/[H_3O^+]^4 [Cl^-]^2 [Mn^2+] [H_2O]^2[Cl_2]/[H_2O^+]^4 [Cl^-]^2 The equilibrium constant K_c for the reaction PCl_3(g) + Cl_2(g) doubleheadarrow PCl_5(g) is 49 at 230 degree C. If 0.70 mol of PCl_3 is added to 0.70 mol of Cl_2 in a 1.00-L reaction vessel at 230 degree C, what is the concentration of PCl_3 when equilibrium has been established? 0.049 M 0.11 M 0.30 M 0.59 M 0.83 M

Explanation / Answer

             = 446.52 gms. of NO2

11) option a
because endothermic reactions can requires less temprature or decrease in temperature to increase the rate of reaction

12)
Kp = pHI^2/(pH2 * pI2)
Kp = 10^2/(1*1)
Kp = 100
given Kp = 10
so option C is correct
13) it is a exothermic reaction so the temperature increases equilibrium shifted towards left side (reversible reaction)
    it favours H2 and Br2 formation

so option C is correct
14) 4H3O^+(aq) + 2Cl^-(aq) + MnO2(s) <....> Mn^+2(aq) + 6H2O (l) + Cl2(g)

option b is correct

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