1. The following reaction is 4 order overall and 1 order in [A]. Determine the missing exponents, a and b.
A(g) + B(g) → c(g) + D(g)
Rate: k[A]a [B]b
2. A given compound decays according to a first order reaction with a half-life of 8.5 minutes. How long will it take for 87 5% to decay?
3. Sketch a potential energy diagram for the following numbers: Eu(forward) : 250 kJ, AH :78 kJ. Find and label Eu(reverse).
4. For each change imposed on the following reaction, choose whether the equilibrium will shift to the right, left, or neither. Circle your choice.
C(s) + 2NzO(g)↔COz(g) + 2Nz(g); AH: ?
a. Remove C(s) (Left, Right, No Change)
b. Add Nz (Left, Right, No Change)
c. Decrease Pressure (Left, Right, No Change)
d. If the amount of NzO increases with heating, is the reaction exothermic or endothermic? (Exothermic, Endothermic)
5. Using the data provided, determine the rate law for the reaction and find the rate constant.
A(aq) +B(aq) → C(g) +D(l)
Run IAI tBt Rate
1 0.200 0.0100 5.4 x 10-7
2 0.200 0.0200 10.8 x 10-7a
J 0.200 0.0400 21.5 x 10'7
4 0.200 0.0600 32.3 x l0'7
5 0.0202 0.200 1.08 x 10-7
6 0.4404 a.200 4.32 x l0-7
7 0.0606 0.200 9.72 x l0'7
8 0.0808 0.200 17.3 x l0'?
6. The decay constant for a certain first order decay is 115 /s or s-1. Find the half life.
7. 0.300 mol No and 0.300 mol o: are initially placed in a reaction vessel. At equilibrium, 0.008 mol NO is left. Calculate the equilibrium amounts of NOz(g) and oz(g)
NO(g) + O:(g) T → NOz(g) + Oz(e)
8. 0.400 mol IBr(g) are initially put in a2.00 L vessel. Find the equilibrium concentrations of all species if K.:0.0036'
2IBr(g) → Iz(g) + grz(g)