What volume of O2 (at 1.064 atm and 21.1
oC) is produced by the decomposition of 6.48 kg of
HgO?
2 HgO(s) --> 2 Hg(l) + O2(g)
V = ___ L
Automobile airbags are inflated by the rapid decomposition of
sodium azide (NaN3).
2 NaN3(s) --> 2 Na(s) + 3 N2(g)
What volume of N2 gas, at 1.02 atm and 23.7
oC, is produced by the complete decomposition of 129.3 g
of sodium azide?
V = ___ L
Calculate the...
PART A.Identify the proper form of the equilibrium-constant
expression for the equation
N2(g)+O2(g)⇌2NO(g)
1.K=[NO][N2][O2]
2.K=[NO]2[N2][O2]
3.K=[N2][O2][NO]2
4.K=2[NO][N2][O2]
PART B. The equilibrium-constant of the reaction
NO2(g)+NO3(g)⇌N2O5(g)
is K=2.1×10−20. What can be said about this
reaction?
1.At equilibrium the concentration of products and reactants is
about the same.
2.At equilibrium the concentration of products is much greater
than the concentration of reactants.
3.At equilibrium the concentration of reactants is much greater
than that of products.
4.There are no reactants left over once...
A mixture of H2(g) and O2 (g) at 1.50 atm
in a rigid container at temperature T is ignited. The remaining
gas, which is entirely H2 (g) exerts a pressure of 0.30
atm at tempertaure T. Assume that the gases are ideal and the
H2O(l) formed in the combustion reaction
takes up negligible volue in the container. Determine the mole
fraction of O2(g) in the original mixture.
A mixture of H2(g) and O2 (g) at 1.50 atm
in a rigid container at temperature T is ignited. The remaining
gas, which is entirely H2 (g) exerts a pressure of 0.30
atm at tempertaure T. Assume that the gases are ideal and the
H2O(l) formed in the combustion reaction
takes up negligible volue in the container. Determine the mole
fraction of O2(g) in the original mixture.
Use the data below for O2 gas at 273.15 K:
P (atm)
Vm
(dm3/mol)
(g/dm3)
0.750000
29.8649
1.07144
0.500000
44.8090
0.714110
0.250000
89.6384
0.356975
a. Under what pressure conditions will O2 act most
like an ideal gas and obey the ideal gas law?
b. Rearrange the ideal gas law to solve for the gas law
constant, R.
Consider the equilibrium
N2(g) + O2(g) ⇄ 2 NO(g)
At 2300 K the equilibrium constant K = 1.7 × 10-3. Suppose that
0.0150 mol NO(g), 0.250 mol N2(g), and 0.250 mol O2(g) are placed
into a 10.0-L flask and heated to 2300 K. The system is not at
equilibrium. Determine the direction the reaction must proceed to
reach equilibrium and the final equilibrium concentrations of each
species.
to the right
to the left
[N2] =____ mol/L
[O2] = ____mol/L
[NO]...
(a) Find ∆G◦ and K at 298.15 K for the gas-phase reaction
2 SO2(g) + O2(g) 2 SO3(g)
(b) If a stoichiometric mixture of SO2 and O2 is allowed to come
to equilibrium at 298.15 K and 1.000bar, find the partial pressure
of SO2.
1.The total pressure of a mixture of O2(g) and H2(g) is 1.95
atm. The mixture is ignited and the resulting water is removed. The
remaining mixture is pure H2(g) and exerts a pressure of 0.210atm
when measured at the same temperature and volume as the original
mixture. What were the mole fractions of O2(g) and H2(g) in the
original mixture?