Answer: The partial pressure of oxygen is 76.56 atm , partial pressure of carbon dioxide is 10.44 atm and the total pressure is 87 atm.
Explanation:
According to the ideal gas equation:'
P = Pressure of the gas = ?
V= Volume of the gas =
T= Temperature of the gas = 10°C = 373 K
R= Gas constant = 0.0821 atmL/K mol
n= moles of gas= 0.25 +0.034 = 0.284 moles
= mole fraction of oxygen=,
=mole fraction of carbon dioxide=
partial pressure of oxygen =
partial pressure of carbon dioxide=
The partial pressure of oxygen is 76.56 atm , partial pressure of carbon dioxide is 10.44 atm and the total pressure is 87 atm.
Answer:
[H₃O⁺] = 1.4 × 10⁻⁹ M.
Explanation:
NH₄Cl is a salt that dissolves well in water. The 2.5 M NH₄Cl will give an initial NH₄⁺ concentration of 2.5 M.
NH₃ is a weak base. It combines with water to produce NH₄⁺ and OH⁻. The opposite process can also take place. NH₄⁺ combines with OH⁻ to produce NH₃ and H₂O. The final H₃O⁺ concentration can be found from the OH⁻ concentration. What will be the final OH⁻ concentration?
Let the increase in OH⁻ concentration be x. The initial OH⁻ concentration at room temperature is 10⁻⁷ M.
Construct a RICE table for the equilibrium between NH₃ and NH₄⁺:
.
The value for ammonia is small. The value of x will be so small that at equilibrium, and .
.
.
.
Again, at room temperature.
Answer:
Basic
Explanation:
pH = -log[H⁺] = - log(1.87 x 10⁻¹¹) = 10.73 (basic solution)