If the reaction quotient, Q, is greater than K in a gas phase reaction, then the
ID: 966199 • Letter: I
Question
If the reaction quotient, Q, is greater than K in a gas phase reaction, then the chemical system has reached equilibrium. the temperature must be increased for the reaction to protected in the forward direction. the reaction will proceed in the forward direction until equilibrium is established. the reaction will proceed in the backward direction until equilibrium is established. the reaction will proceed in the direction that increases the number of gas phase particles. At some temperature, the reaction. 2 NH_2(g) N_2(g) + 3 H_2 (g) has k_g = 0.64. At equilibrium, it is found that [NH_3] = [H_2]. What is [H_2] when this equilibrium is reached? 0.80 M 0.64 M 1.0 M 2.4 M 0.41 M Given the equilibrium constants for the following reactions: What is K for the system. 2CU(s) + O_2(g) 2CuO(s) equivalent to? (K_2)^2/(K_1) K_1 middot K_2 (K_1)(K_3)^16 Which one is the conjugate acid of bisulfate ion, HSO_4^-? HSO_4^H_2SO_4 SO_4^2 - HSO_4 H_3O^- In which ONE of the following systems at equilibrium will an increase in the pressure brought about by decreasing the volume of the container have no effect on the concentrations of products and reactants? H_2(g) + F_2 (g) 2HF(g) N_2(g) + 3 H_2(g) 2 NH_3(g) CaCO_3(s) CaO(s) + CO_2(g) 2 NOBr(g) 2 NO(g) + Br_2(g) 2 H_2O (g) + O_2(g) 2 H_2O(g) For the reaction 2HI(g) H_2(g) + I_2(g), K_c = 0.290 at 400 K. If the initial concentrations of Hl, H_2, and l_2 are all 1.50 Times 10^-3 M at 400 K, which ONE of the following statements is correct? The concentrations of HI and l_2 increase as the system approaches equilibrium. The concentrations of H_2 and l_2 increase as the system approaches equilibrium. The system is at equilibrium. The concentrations of H_2 and HI decrease as the system approaches equilibrium. The concentration of HI increases as the system approaches equilibrium.Explanation / Answer
6) If Q > Kc, it means the reaction will go towards reactants
Q = product of concentration of product / product of concentration of reactant
so if Q is more then the reaction will favour reactants. [option C]
7) Kc = 0.64
Kc = [N2] [H2]^3 / [NH3]^2
At equilibrium [NH3] = [H2] = [N2] =x
Kc = x^4 / x^2
0.64 = x^2
x = 0.8
So concentration of H2 = 0.80 M
8) Given
4Cu(s) + O2(g) --> 2Cu2O (s) K1.....................1
2CuO (s) --> Cu2O +1/2O2(g) K2....................2
2Cu(s) + O2 -> 2CuO(s) K .............................3
Now we can obtain equation from equation 1 and 2 as
1/2( Equation 1 ) - equation 2
so the value of K = (K2)1/2 / K1
9) The conjugate acid is obtained by adding proton to given base
HSO4- + H+ --> H2SO4 (conjugate acdi)
10) there will be no effect on pressure or volume if the number of moles of gaseous compounds is same on both reactant and product side
Answer : H2(g) + F2(g) --> 2HF (g) [ two moles each side]
11) 2HI --> H2 + I2
The concentration of H2 and I2 increases as the system approaches equilbrium