Which statements are true in the following choice? select all that apply. question 18 options: consider the following reaction.2so2(g) + o2(g) -> 2so3(g),the expression of its kc, the equilibrium constant using concentrations in function of its kp, the equilibrium constant using pressures is kc = kp x (rt)^ 1.consider the following reaction.2so2(g) + o2(g) -> 2so3(g),the expression of its kc, the equilibrium constant using concentrations in function of its kp, the equilibrium constant using pressures is kc = kp / (rt)^-1.consider the following reaction: na2co3(s) + 2hno3(aq) < -> 2nano3(aq) + h2o(l) + co2(g)the expression of the equilibrium constant for the reaction is k = [nano3] ^2 x [co2] / [hno3]^2.because the reaction is a heterogeneous equilibrium, pure liquids and solids are not included in the expression of the equilibrium constant. consider the following reaction: na2co3(s) + 2hno3(aq) < -> 2nano3(aq) + h2o(l) + co2(g)the expression of the equilibrium constant for the reaction is k = [na2co3] x [hno3]^2 / [nano3] ^2 x [co2].because the reaction is a heterogeneous equilibrium, pure liquids and solids are included in the expression of the equilibrium constant. note: whenever appropriate, use the sign x for multiplication operations. a chemical reaction can be considered as a combination of several reactions. its equilibrium constant can be expressed as a combination of the equilibrium constants of the component reactions. for example the reaction : equation 1: h2(g) + co2(g) < => co(g) + h2o(g) with k1 for equilibrium constantk1 = [co]x[h2o]) / [h2]x[co2], can be viewed as a combination of the following reactions: equation 2: co(s) + h2o(g) < => coo(s) + h2(g) with k2 for equilibrium constantk2 = [h2]/[h2o] andequation 3: coo(s) + co(g) < => co(s) + co2(g) with k3 for equilibrium constantk3 = [co2]/[co].close examination of the right side of the expression of k1 shows it is made of a combination of k2 and k3. the expression of k1 in terms of k2 and k3 becomes: k1 = (1/k2) x (1/k3)note: whenever appropriate, use the sign x for multiplication operations. a chemical reaction can be considered as a combination of several reactions. its equilibrium constant can be expressed as a combination of the equilibrium constants of the component reactions. for example the reaction : equation 1: h2(g) + co2(g) < => co(g) + h2o(g) with k1 for equilibrium constantk1 = [h2]x[co2] / [co]x[h2o]), can be viewed as a combination of the following reactions: equation 2: co(s) + h2o(g) < => coo(s) + h2(g) with k2 for equilibrium constantk2 = [h2]/[h2o] andequation 3: coo(s) + co(g) < => co(s) + co2(g) with k3 for equilibrium constantk3 = [co2]/[co].close examination of the right side of the expression of k1 shows it is made of a combination of k2 and k3. the expression of k1 in terms of k2 and k3 becomes: k1 = k2 / k3