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Determine the rate law for the reaction below. Experiment [Q2] (M) [J2] (M) Rate (M/s) 1 0.786 0.548 4.48 x 10-2 2 1.572 1.096 8.96 x 10-2 3 1.572 0.548 4.48 x 10-2 4 0.393 0.274 2.24 x 10-2

Which of the following statements is/are correct about the graph shown below?   The graph represents a strong acid/strong base titration The pH at the equivalence point in approximately 8.25 The pKa is approximately 8.25

Which of the following statements is/are true about graphs regarding rate data below? The half-life, t1/2, is independent of concentration Changing the concentration of A will not affect the rate of the reaction The units for the rate constant k are s-1

Determine if the following statements about the solubility of a gas are true or false.  The solubility of a gas increases as the strength of the intermolecular forces increases between the solute (gas) and the solvent. [1] The solubility of a gas decreases as temperature increases. [2] The solubility of a gas decreases as pressure increases. [3]

For the following reaction what is the rate of disappearance of X when the rate of appearance of Z is 6.75 x 10-3 M/s? 3X → 2Z + Q

Substance Q decays by 1st order kinetics and has a half-life of 45 s and a rate constant of 1.2 M/s. If Q is initially 0.88 M how much would remain after 5 half-lives?

X2 and Z2 react to give XZ X2 (g) +  Z2 (g) ⇌ 2XZ (g)    KC= 56.18 at 37°C If a 3.00 L flask initially contains 0.00258 mol each of X2 and Z2, find the equilibrium concentration of Z2 in the mixture at 37°C.  

What is the pH of a 1 L buffer solution containing 0.502 M diethylamine, (C2H5)NH, and 0.331 M diethylammonium bromide (C2H5)NH2Br?

Consider the reaction below with Kp = 33.9 at 25o C.  The partial pressure of H2 is measured to be 1.145 atm, partial pressure of F2 is measured to be 1.145 atm, and and partial pressure of HF is measured to be 2.275 atm. Which of the following is true regarding the above system? The reaction proceeds in the forward direction to reach equilibrium The reaction proceeds in the reverse direction to reach equilibrium The reaction is at equilibrium Therefore: 4. The concentration of the reactants will increase, and the concentration of the products will decrease. 5. The concentration of reactants and products will not change. 6. The concentration of products will increase, and the concentration of reactants will decrease.

Identify the Lewis base in the reaction below.