1.Write the equilibrium expression (K) for each of the following gas-phase reactions. a. N2 (g) + 02 (g) = 2N0(g) b. N204(g) = 2N02(g) c. SiH4, (g) + 2Cl2 (g) = SiCI4 (g) + 2H2 (g) d. 2PBr3 (g) + 3Cl2 (g) = 2PCl3 (g) + 3Br2 (g
1.Write the equilibrium expression (K) for each of the following gas-phase
reactions.
a. N2 (g) + 02 (g) = 2N0(g)
b. N204(g) = 2N02(g)
c. SiH4, (g) + 2Cl2 (g) = SiCI4 (g) + 2H2 (g)
d. 2PBr3 (g) + 3Cl2 (g) = 2PCl3 (g) + 3Br2 (g)
2. Write the equilibrium expression (K.) for each reaction above
3. At 327°C, the equilibrium concentrations are [CH3OH] = 0.15 M
[CO] = 0.24 M, and H2 = 1.1 M for the reaction
CH3OH(g) = CO(g) + 2H2 (g)
Calculate (Kp)at this temperature.
4. The equilibrium constant is 0.0900 at 25°C for the reaction
H2O(g) + Cl2(g) = 2HOCl(g)
For which of the following sets of conditions is the system at
equilibrium? For those that are not at equilibrium, in which
direction will the system shift?
a. A 1.0-L flask contains 1.0 mole of HOCI, 0.10 mole of
Cl2O, and 0.10 mole of H2O.
b. A 2.0-L flask contains 0.084 mole of HOCI, 0.080 mole
of Cl2O, and 0.98 mole of H2O.
c. A 3.0-L flask contains 0.25 mole of HOCl, 0.0010 mole
of ClO, and 0.56 mole of H2O.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
