In the collision model, which factor is most sensitive to changes in temperature?

The following three mechanisms have been proposed for the reaction 2H2(g) + 2NO(g) → N2(g) + 2H2O(g). Mechanism I H2 + NO → H2O + N (slow) N + NO → N2 + O (fast) O + H2 → H2O (fast) Mechanism II 2NO ⇌ N2O2 (fast equilibrium) N2O2 + H2 → N2O + H2O (slow) N2O + H2 → N2 + H2O (fast) Mechanism III H2 + 2NO → N2O + H2O (slow) N2O + H2 → N2 + H2O (fast) The experimentally determined rate law is found to be rate = k[H2][NO]2. Given the three proposed mechanisms, which mechanism(s) cannot be correct?

Consider the following reaction: 2 NO(g) + O2 (g) ⇌ 2 NO2 (g) Kp = 5.0 x 1012 Some NO2 (g) is added to an empty container, which is then sealed. What is true regarding the concentration of each gas at equilibrium?

The gas phosphine, PH3, decomposes by the following reaction: 2 PH3 (g) ⇌ 2 P(s) + 3 H2 (g). In an experiment, pure phosphine was placed in a rigid, sealed flask of volume 1.00 L at 0.64 atm pressure and 298 K. After equilibrium was attained, the total pressure in the flask was measured to be 0.93 atm. Calculate Kp for the reaction at this temperature.

Taking ion-pairing into account, which of the following solutions should have the smallest ΔTf?

The reaction A2 → B + C obeys the rate law: rate = (1.0 x 10-2 min-1) [A2] at 298 K. How long will it take for the reaction to reach 60% completion?

I. A Lewis base is defined as a substance that acts as an electron pair donor . II. Which of the following species can act as a Lewis base, AlBr3 or PBr3?

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. 2H2(g) + 2Br2(g) ⇌ 4 HBr(g) Kc = ? 2 HBr(g) ⇌ H2(g) + Br2(g) Kc = 2.6 x 10-5

In the Haber-Bosch process, iron metal is typically used to catalyze the following reaction: N2(g) + 3 H2(g) ⇌ 2 NH3(g) Identify the following statements as either true or false: I. Iron metal acts as a homogeneous catalyst for this reaction. II. The activation energy (Ea) for the overall reaction is lowered when a catalyst is used. III. The energy change (ΔE) for the overall reaction is unchanged when a catalyst is used.

Consider the equilibrium associated with the elementary reaction Cl2(g) ⇌ 2 Cl(g). If a mixture of products and reactants at equilibrium is disturbed by reducing the volume of the reaction vessel, while maintaining a constant temperature, how will the rates of the forward and reverse reaction change immediately after the disturbance?

Consider the following reaction: CO2(g) + C(graphite) ⇌ 2 CO(g) A reaction mixture initially contains graphite, 0.56 atm CO2 and 0.32 atm CO. If Kp for the reaction at this temperature is 4.25, how will the concentration of each substance change in order to achieve equilibrium? I. CO2(g) II. CO(g)

A student mixed together 50.0 g chloroform (CHCl3) and 50.0 g of benzene (C6H6) at 25°C. What is the vapor pressure of the chloroform above the mixture? Assume the solution behaves ideally. The vapor pressure of chloroform and benzene at 25°C is 172.0 torr and 94.4 torr, respectively. (MW of CHCl3 = 119.38 g/mol; C6H6 = 78.11 g/mol)

The boiling point of acetone is 56.00°C. 3.75 g of CaCl2 was dissolved in 121 mL of acetone. What is the boiling point of the solution? Assume no ion pairing. (MW: acetone = 58.08 g/mol; CaCl2 = 110.98 g/mol, Kb = 1.67°C/m, density of acetone = 0.784 g/mL) Round your answer to TWO decimal places

The reaction H2 (g) + I2 (g) → 2 HI (g) follows the rate law k[H2 ][I2 ]. Which of the following changes will increase the rate of the reaction, but not change the rate constant?

A 0.100 m solution of BaSO4 has a __________ boiling point than a 0.100 m solution of NaCl because the extent of ion pairing is greater for __________ in solution.

Which of the following is the best description of why ion pairing is likely to occur in a solution of MgSO4 dissolved in water?

A biochemist is investigating a form of hemoglobin. She dissolves 21.5 mg of the sample in enough water to make a 1.50 mL solution at 5.0°C. The measured osmotic pressure is 3.61 torr. What is the molar mass of the hemoglobin?

What is the mole fraction of heptane (C7H16) in the vapor phase of a solution of 0.226 mol CBr4 and 0.271 mol C7H16 at 100°C? (Vapor pressures of pure substances at 100°C: CBr4 = 47.2 torr; C7H16 = 493.19 torr)

Consider the solute-solvent interactions for the different solutions: I. LiF in CH3Cl II. CH2Cl2 in benzene (C6H6) III. Water in methanol (CH3OH) Rank them from strongest to weakest.

The following rate data were obtained at 25oC for the oxidation of Cr3+ to CrO42- using Ce4+ in a buffered solution. What is the rate-law expression for the reaction?

Which of the following liquids is immiscible with water?

A 1.0 L evacuated tank is charged with HI(g) to a pressure of 1.0 atm and 793 K. Some of the HI(g) forms H2(g) and I2(g) according to the following equilibrium: 2 HI(g) ⇌ I2 (g) + H2 (g) Kp = 1.6 x 10-2 What is the partial pressure (in atm) of HI at equilibrium? Enter only the numerical value of atm and do not include units.

For the following reaction, 3.000 mole of A2 are placed in a 2.000 L flask and allowed to reach equilibrium, at 25oC. At equilibrium 1.050 moles of A2 remains. What is the value of Kc ? 3 A2 (g) ⇌ 2 A3 (g)

According to the following reaction, if 0.30 mol NOCl and 0.50 mol Cl2 are introduced into a 1.0 L container, how much NO is present at equilibrium? 2 NOCl(g) ⇌ 2 NO(g) + Cl2 (g) K = 1.6 x 10-5

A reaction is started with both reactants and products and proceeds in the reverse direction to reach equilibrium. Which of the following statements best describes why the reaction proceeds in the reverse direction?

Zinc hydroxide is not appreciably soluble in water. For the reaction at equilibrium, K is __________ and __________ are favored. Zn(OH)2 (s) ⇌ Zn2+ (aq) + 2 OH- (aq)

Which of the following reactions lies more to the right at equilibrium?

Consider the following reaction taking place in a sealed 1.00 L container: 2 NO(g) + Br2(g) ⇌ 2 NOBr(g) Kc = 2.0 at 298K The initial conditions are [NO(g)] = 0.350, [Br2(g)] = 0.750, and [NOBr(g)] = 1.500. What happens as the reaction proceeds toward equilibrium?