Reference no: EM132553618
1. Relate the rate of decomposition of NO2 to the rate of formation of Oz for the following reaction:
2 NO2(g) → 2 NO(g) + O2 (9)
2. Relate the rate of disappearance of iodine vapour to the rate of formation of hydrogen iodide in the following reaction:
H2(g) + 12(g) → 2 H1 (9)
3. Dinitrogen pentoxide decomposes according to the following equation:
2 N205 (9) ? 4 NO2(g) + O2(g)
If the concentration of N205 changes from 1.24 x 10-2 mol/L to 9.30 x 10-3 mol/L during an interval of 600 s, calculate the average rate of reaction of N2O5.
4. The iodide ion is oxidized by hypochlorite ion in basic solution according to the following equation:
l-(aq) + CeO- (aq) → CE (aq) + 10- (aq)
If the iodide ion concentration changed from 1.69 x 10-3 mol/L to 1.01 x 10-3 mol/L during an interval of 6.00 s, calculate the average rate of reaction of iodide ion.
5. Ammonium nitrite decomposes in solution according to the following equation:
NH4NO2 (aq) → N269) + 2 H2O (0)
a. If the concentration of ammonium nitrite changes from 0.500 mol/L to 0.432 mol/L during an interval of 3.00 hours,
Calculate the average rate of decomposition of ammonium nitrite.
b. Calculate the average rate of formation of water.
6. Iron (III) chloride is reduced by tin (II) chloride according to the following equation:
2 FeCl3 (aq) + SnCl2 (aq) → 2 FeCl2 (aq) + Sn Cla (aq)
a. If the concentration of iron (III) chloride changed from 0.03586 mol/L to 0.02638 mol/L during an interval of 4.00 min,
Calculate the average rate of reaction of FeCl3.
b. Calculate the average rate of reaction of Sn Cla.
7. If Ea = 200.0 kJ, calculate the change in the rate constant if the temperature of a system is raised from 20.0°C to 25.0°C.
8. The temperature of a system is raised from 20.0°C to 25.0°C. If Ea = 200 kJ, calculate the change produced by the use of a catalyst that lowers the activation energy by 10.0%.
9) Consider the following reaction. CH3CHO (g) → CH4 (9) + CO (9)
The rate constant for the decomposition is 1.05 x 10-3 mol1/2/L 1/2.s at 759 K & 2.14 x 10-2 mol1/2/L112.s at 836 K. What is the activation energy for the reaction?
10. Observe the following reaction: 2 NOCE (9) ? 2 NO(g) + Cl2(g)
The rate constant is 9.30 x 10-6 5-1 at 350 K & 6.90 x 104 3-1 at 400 K. Calculate the activation energy for the reaction & determine by what factor the rate increased.
11) The rate of a particular reaction doubles when the temperature is increased from 25.0°C to 35.0°C. Calculate the activation energy for this reaction.
12) For the decomposition of HI, the rate constant is 2.69 x 10-3 L/mol.s at 440 K & 6.21 x 10-3 L/mol.s at 460 K. Calculate the activation energy for the reaction & then calculate the value of the rate constant at 500 K.