Answer:
3.9
Explanation:
Let's consider the following reaction at equilibrium.
CO(g) + Cl₂(g) ↔ COCl₂(g)
We can find the pressures at equilibrium using an ICE chart.
CO(g) + Cl₂(g) ↔ COCl₂(g)
I 0.96 1.15 0
C -x -x +x
E 0.96-x 1.15-x x
The sum of the partial pressures is equal to the total pressure.
pCO + pCl₂ + pCOCl₂ = 1.47
(0.96-x) + (1.15-x) + x = 1.47
2.11 - x = 1.47
x = 0.64
The pressures at equilibrium are:
pCO = 0.96 - x = 0.32 atm
pCl₂ = 1.15 - x = 0.51 atm
pCOCl₂ = x = 0.64 atm
The pressure equilibrium constant (Kp) is:
Kp = pCOCl₂ / pCO × pCl₂
Kp = 0.64 / 0.32 × 0.51
Kp = 3.9
Answer:
A compound
Explanation:
Chemical compound can be regarded as any substance made up of identical molecules which consists atoms of two or more than two chemical elements. For example four hydrogen atoms bonds with a carbon atom to give methane molecule which is a compound. It should be noted that A compound is a new substance with unique chemical and physical properties formed when two or more elements are chemically bonded during a physical reaction.
<span>A fast moving stream of air has a lower air pressure than a
slower air stream. As the stream of air moved over the
top of the paper, the air pressure over the paper dropped. The
air pressure underneath the paper stayed the same. The
greater air pressure underneath lifted the paper strip and it
rose. The idea that a moving air stream has lower air pressure
than air that is not moving is called “Bernoulli’s Principle”.
</span>The
force of the moving air underneath the balloon was enough to
hold it up. The weight added by the paper clip prevents
the balloon from going too high. But that is only part
of the story. The balloon stays inside the moving stream
of air because the pressure inside is the air stream is lower
than the still air around it. As the balloon moves toward the
still air outside of the air stream, the higher pressure of
the still air forces the balloon back into the lower pressure
of the air stream. Bernoulli’s Principle at work again!
It has to be NH3 (ammonia)
the rest are definitely acidic
Answer:
The molar mass of the liquid 62.89 g/mol
Explanation:
Step 1: Data given
Mass of the sample = 0.1 grams
Temperature = 70°C
Volume = 750 mL
Pressure = 0.05951 atm
Step 2: Calculate the number of moles
p*V = n*R*T
n = (p*V)/(R*T)
⇒ with n = the number of moles gas = TO BE DETERMINED
⇒ with p = The pressure = 0.05951 atm
⇒ with V = The volume of the flask = 750 mL = 0.750 L
⇒ with R = The gasconstant = 0.08206 L*atm/K*mol
⇒with T = the temperature = 70 °C = 343 Kelvin
n = (0.05951 *0.750)/(0.08206*343)
n = 0.00159 moles
Step 3: Calculate molar mass
Molar mass = mass / moles
Molar mass =0.1 gram / 0.00159 moles
Molar mass = 62.89 g/mol
The molar mass of the liquid 62.89 g/mol
