Barrons SAT Subject Test Chemistry, 13th Edition

(T, T) Both statements are true, but the second does not explain the first, and there is no cause and effect relationship. Entr ...

(T, F) In the decomposition of HgO, Hg and O 2 are the products. The equation is 2HgO → 2Hg + O 2 (g) It is not always true th ...

9. Rates of Chemical Reactions 1. (1) Nature of the reactants (2) Surface area exposed (3) Concentrations (4) Temperature (5) Pr ...

(D) When a catalyst is added to a reaction, it is used to either increase or decrease the activation energy needed for the reac ...

(A) When the concentration of reactants is increased, the number of collisions between reactants is directly affected because t ...

(A) At the beginning of a reaction, the reaction rate of the reactants is the highest because their concentration is the highes ...

(D) For the reaction aA + bB → AB, the reaction rate law would give the expression of r as proportional to [A]a[B]b. ...

10. Chemical Equilibrium 1. (C) The correct setup of Keq is the product of the concentration of the products over the products o ...

(D) The concentrations in an expression of the equilibrium constant are given in moles/liter (mol/L). ...

(A) This reaction is the equilibrium between a precipitate and its ions in solution. Because BaSO 4 is a solid, it does not app ...

(C) This is the K expression of water. ...

(A) Because the pH is defined as the negative of the log of the H+ concentration, it is –(log of 10–4), which is –(–4) or 4. ...

(C) pH + pOH = 14. In this problem, the pOH = –log [OH] = –log [10–4] = –(–4) = 4. Placing this value in the equation, you have ...

(D) For Keq to be a small value, the numerator of the expression must be small compared with the denominator. Because the nume ...

(A) In the reaction for the formation of ammonia, N 2 + 3H 2 ↔ 2NH 3 + heat (at equilibrium), an increase in pressure will cau ...

(A) Only the changing of the temperature of the equilibrium reaction will change the K of the equilibrium given at the starting ...

(B) Because there already is a concentration of (OH)– ions from the NaOH in solution, this common ion effect will decrease the ...

(A) When enthalpy is negative and entropy is positive, the free energy is always negative. ...

(C) When enthalpy is positive and entropy is positive, the free energy is negative at high temperatures. ...

(B) When enthalpy is negative and entropy is negative, the free energy is negative at lower temperatures. ...