Question
In: Chemistry
An empty 5.00-L flask is charged with 0.250 g of pure H2S(g), at 25 ∘C. What...
An empty 5.00-L flask is charged with 0.250 g of pure H2S(g), at 25 ∘C.
What is the initial pressure of H2S(g) in the flask? 3.59*10^-2 atm
In addition to the H2S already present in the flask, solid NH4HS is added until there is excess unreacted solid remaining.
a) What are the partial pressures of NH3 and H2S at equilibrium, that is, what are the values of PNH3 and PH2S, respectively?
b)What is the mole fraction, χ, of H2S in the gas mixture at equilibrium?
c)What is the minimum mass of NH4HS that must be added to the 5.00-Lflask when charged with the 0.250 g of pure H2S(g), at 25 ∘C to achieve equilibrium? Express your answer numerically in grams.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
A 5.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure. What is the final...
A 5.00-L flask contains nitrogen gas at 25°C and 1.00 atm
pressure. What is the final pressure in the flask if an additional
2.00 g of N2 gas is added to the flask and the flask cooled to
-55°C?
a.) 0.987 atm
b.) 1.35 atm
c.) 1.84 atm
d.) 0.255 atm
A flask is charged with 1.660 atm of N2O4(g) and 1.01 atm NO2(g) at 25°C. The...
A flask is charged with 1.660 atm of N2O4(g) and 1.01 atm NO2(g)
at 25°C. The equilibrium reaction is given in the equation below.
N2O4(g) 2NO2(g) After equilibrium is reached, the partial pressure
of NO2 is 0.512 atm. (a) What is the equilibrium partial pressure
of N2O4? (b) Calculate the value of Kp for the reaction. (c) Is
there sufficient information to calculate Kc for the reaction? No,
because the value of Kc can be determined experimentally only. Yes,
because...
At 100∘C, Kc = 4.72 for the reaction 2NO2(g)⇌N2O4(g). An empty 10.0 L flask is filled...
At 100∘C, Kc = 4.72 for the reaction
2NO2(g)⇌N2O4(g).
An empty 10.0 L flask is filled with 2.30 g of NO2at 100∘C.
1) What is the total pressure in the flask at equilibrium?
A 1.00 L flask is filled with 1.45 g of argon at 25 ∘C. A sample...
A 1.00 L flask is filled with 1.45 g of argon at 25 ∘C. A sample
of ethane vapor is added to the same flask until the total pressure
is 1.000 atm
What is the partial pressure of argon, PAr, in the
flask? What is the partial pressure of ethane, Pethane, in
the flask?
A 1.00 L flask is filled with 1.20 g of argon at 25 ∘C. A sample...
A 1.00 L flask is filled with 1.20 g of argon at 25 ∘C. A sample
of ethane vapor is added to the same flask until the total pressure
is 1.450 atm . What is the partial pressure of argon, PAr,
in the flask?
A 1.00 L flask is filled with 1.45 g of argon at 25 ∘C. A sample...
A 1.00 L flask is filled with 1.45 g of argon at 25 ∘C. A sample
of ethane vapor is added to the same flask until the total pressure
is 1.450 atm .
What is the partial pressure of ethane, Pethane, in the flask?
Express your answer to three significant figures and include the
appropriate units.
Consider a 5.00-L tank containing 375 g of Ar at a temperature of 25 °C. (a)...
Consider a 5.00-L tank containing 375 g of Ar at a temperature
of 25 °C.
(a) Calculate the pressure in the tank using both the ideal gas law
and the van der Waals equation.
(b) Which correction term, a(n/V)2 or bn, has the great- est
influence on the pressure of this syste
A flask is charged with 1.350 atm of N2O4(g) and 1.00 atm of NO2(g) at 25...
A flask is charged with 1.350 atm of N2O4(g) and 1.00 atm of
NO2(g) at 25 ∘C, and the following equilibrium is achieved:
N2O4(g)⇌2NO2(g)
After equilibrium is reached, the partial pressure of NO2 is
0.517 atm.
Part A:
What is the partial pressure of N2O4 at equilibrium?
Express the pressure to three significant figures and include
the appropriate units
Part B:
Calculate the value of Kp for the reaction.
Express your answer to three significant figures.
Part C:
Calculate the...
If the partial pressure of hof in a 1.00-L flask is initially at 25 °C, what...
If the partial pressure of hof in a 1.00-L flask is initially at
25 °C, what are the total pressure in the flask and the partial
pressure of after exactly 35 minutes? After 57 min?
A 1.100−L flask at 25∘C and 1.00 atm pressure contains CO2(g) in contact with 100.0 mL...
A 1.100−L flask at 25∘C and 1.00 atm pressure contains
CO2(g) in contact with 100.0 mL of a saturated aqueous solution in
which [CO2(aq)] = 3.29×10−2 M.
a) What is the value of Kc at 25∘C for the
equilibrium CO2(g)⇌CO2(aq)
Answer: Kc = 0.804
b) If 0.01400 M of radioactive 14CO2 is
added to the flask, how many moles of the 14CO2 will be
found in the gas phase and in the aqueous solution when equilibrium
is reestablished?
[Hint: The radioactive 14CO2 distributes itself
between the two phases in exactly the same...
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