Question

#5.133

A mixture of NH3(*g*) and N2H4(*g*) is placed in a
sealed container at 320 K . The total pressure is 0.53 bar . The
container is heated to 1200 K at which time both substances
decompose completely according to the equations
2NH3(*g*)→N2(*g*)+3H2(*g*) ;
N2H4(*g*)→N2(*g*)+2H2(*g*) . After
decomposition is complete the total pressure at 1200 K is found to
be 4.5 bar.

Find the percent (by volume) of N2H4(*g*) in the original
mixture. (Assume two significant figures for the temperature.)

Answer #1

0.51 atm at 320K, would be (0.51 atm) x (1200 / 320) =

Let z be the partial pressure (in atm) of N2H4 in the original
mixture.

Then 0.51-z is the partial pressure of NH3 in the original
mixture.

N2H4 → N2 + 2 H2

So z atm of H2N4 would produce 3z of products.

2 NH3 → N2 + 3 H2 [That is: 1 mol of NH3 produces 2 mol of
products.]

So 0.51-z of NH3 would produce 1.02 - 2z of products.

(4.5 atm) x (320 / 1200) = 1.2 atm at 320K

Add the two expressions for partial pressure of products and set it
equal to the total pressure of products at the same
temperature:

3z + (1.02 - 2z) = 1.2 atm

Solve for z algebraically:

z = 0.18 atm originally

(0.18 / 0.51) = 0.35 = 35% N2H4 by partial pressure, and so 35%
N2H4 by volume

Hope this helps

At 500 K, a 10.0 L equilibrium mixture contains 0.424 mol N2,
1.272 mol H2, and 1.152 mol NH3. The mixture is quickly chilled to
a temperature at which the NH3 liquefies, and the NH3(l) is
completely removed. The 10.0 L gaseous mixture is then returned to
500 K, and equilibrium is re-established.
How many moles of NH3(g) will be present in the new equilibrium
mixture?
N2(g)+3H2(g)→2NH3(g)
Express your answer to three significant figures and include the
appropriate units.

When 0.0430 mol of HI is heated to 500 K in a 5.00 L sealed
container, the resulting equilibrium mixture contains 2.85 g of HI.
Calculate Kc and Kp for the following decomposition reaction. 2 HI
(g) H2 (g) + I2 (g)

Constants | Periodic Table
A sample of {\rm SO}_{3} is introduced into an evacuated sealed
container and heated to 1233 {\rm K}. The following equilibrium is
established:
{\rm{2 SO}}_3 {\rm{(}}g{\rm{) }} \rightleftharpoons {\rm{ 2
SO}}_2 {\rm{(}}g{\rm{) + O}}_2 {\rm{(}}g{\rm{)}}.
The total pressure in the system is found to be 3.0 \rm bar and the
mole fraction of {\rm O}_{2} is 0.12.
Part A
Find K.
Express your answer using two significant figures.

1.) The equilibrium constant for the chemical equation
N2(g)+3H2(g) <-->
2NH3(g)
is Kp = 1.09 at 209 °C. Calculate the value of the Kc for the
reaction at 209 °C.
2.) At a certain temperature, 0.3411 mol of N2 and 1.581 mol of
H2 are placed in a 1.50-L container.
N2(g)+3H2(g) <-->
2NH3(g)
At equilibrium, 0.1801 mol of N2 is present. Calculate the
equilibrium constant, Kc.
3.) At a certain temperature, the Kp for the decomposition of
H2S is 0.748....

A) Consider the following reaction where Kc
= 0.159 at 723 K.
N2(g) +
3H2(g)
2NH3(g)
A reaction mixture was found to contain
4.94×10-2 moles of
N2(g),
4.07×10-2 moles of
H2(g) and
6.19×10-4 moles of
NH3(g), in a 1.00 liter
container.
The reaction quotient, Qc, equals
__________.
The reaction__________________
A. must run in the forward direction to reach
equilibrium.
B. must run in the reverse direction to reach
equilibrium.
C. is at equilibrium.
B) Consider the following reaction where Kc...

A mixture of CO(g) and O2(g) in a 1.1 −L container at 1.0×103 K
has a total pressure of 2.3 atm . After some time the total
pressure falls to 1.8 atm as the result of the formation of
CO2.
Find the mass (in grams) of CO2 that forms.

37)Into a 15.00-liter container at 25°C are placed 1.00 moles of
O2 gas and 3.00 moles of solid C (graphite). If the carbon and
oxygen react completely to form CO(g), what will be the final
pressure in the container at 25°C? a) 0.274 atm b) 1.00 atm c) 4.89
atm d) 1.63 atm e) 3.26 atm
39) N2 (g) + 3H2 (g) 2NH3 (g). If a 3.4 L flask is first
charged with 1.2 atm of nitrogen, then hydrogen is...

part a
The reaction of nitrogen and hydrogen to produce ammonia:
N2(g) + 3H2(g) ⇌ 2NH3(g) has an equilibrium constant Kc= 1.2 at
375 °C. If the starting concentrations are [H2] = 0.76 M, [N2] =
0.60 M, and [NH3] = 0.48 M, at equilibrium which gases will have
increased in concentration and which will have decreased in
concentration?
a. H2
b. N2
c. NH3
part b
When solid sodium bicarbonate is heated the following
decomposition reaction occurs: 2NaHCO3(s) ⇌...

1) Consider the following reaction where Kc =
7.00×10-5 at 673
K.
NH4I(s) -->
NH3(g) + HI(g)
A reaction mixture was found to contain
5.62×10-2 moles of
NH4I(s),
1.12×10-2 moles of
NH3(g), and
8.37×10-3 moles of
HI(g), in a 1.00 liter container.
Is the reaction at equilibrium?
If not, what direction must it run in order to reach
equilibrium?
The reaction quotient, Qc, equals
(???????)
The reaction ?????
A. must run in the forward direction to reach
equilibrium.
B. must...

Consider the reaction: N2(g) + 3H2(g) → 2NH3(g). At a
particular moment during the reaction hydrogen is being
consumed at a rate of 0.074 M/s. At this moment:
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(b) A what rate (in M/s) is NH3 being produced? {3 points}
(c) Are these average or instantaneous rates? {1 point}
[3] A certain first-order reaction has a rate constant of 1.65
min-1 at 20°C. What is the value of the...

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