Answer:
0.02moles
Explanation:
To answer this question, the general gas law equation is used. The General gas law is:
Pv = nRT
Where; P = standard atmospheric pressure (1 atm)
V = volume (L)
n = number of moles
R = Gas law constant
T = Temperature
For this question; volume = 1.00L, atmospheric pressure (P) = 1 atm, R = 0.0821 L-atm / mol K, T = 600K, n = ?
Therefore; Pv = nRT
n = PV/RT
n = 1 × 1/ 0.0821 × 600
n = 1/49.26
n = 0.0203moles
Hence, there are 0.02 moles of gas.
You just have to convert the mass of water into volume.
To do that you use the density of water, which is about 1.0 g/ ml
So, from the formula of density D = M / V, you get V = M / D
=> V = 2.49 * 10^7 grams / 1.0 g / ml = 2.49 * 10 ^ 7 ml
You can pass that to liters using the conversion factor 1000 ml = 1 l
2.49 * 10^7 ml * 1 l / 1000 ml = 2.49 * 10^4 l = 24,900 l
Answer: 24,900 l
Answer:
because it helps you to understand what’s the most important thing on your ”to - do” list and helps you to get it done. the higher up it is on your list, the more you have to prioritize it to get it dome.
Answer:
[PCl₃] = 0.031M
[Cl₂] = 0.031M
[PCl₅] = 0.969M
Explanation:
Based on the reaction:
PCl₅(g) ⇄ PCl₃(g) + Cl₂(g)
Keq is defined as:
<em>Keq = 1.0x10⁻³ = [PCl₃] [Cl₂] / [PCl₅]</em>
<em>Where [] are equilibrium concentrations of each species</em>
Inital [PCl₅] = 2.0mol / 2.0L = 1M.
In equilibrium:
[PCl₃] = X
[Cl₂] = X
[PCl₅] = 1M-X
Where X is reaction coordinate
Solving for X in Keq:
1.0x10⁻³ = [X] [X] / [1-X]
1.0x10⁻³ - 1.0x10⁻³X = X²
1.0x10⁻³ - 1.0x10⁻³X - X² = 0
X:
X = -0.032M. False solution, there is no negative concentration
X = 0.031M
That means equlibrium concentrations are:
[PCl₃] = 0.031M
[Cl₂] = 0.031M
[PCl₅] = 1-0.031M = 0.969M
<h3>[PCl₃] = 0.031M</h3><h3>[Cl₂] = 0.031M</h3><h3>[PCl₅] = 0.969M</h3>
Answer:
Isopropanol>dichloromethane>1-butene>propane
Explanation:
Stronger intermolecular forces usually correlate with higher boiling points
Boiling points generally increases with molecular weight due to increased strength of dispersion forces
Hydrocarbons exhibit only dispersion forces.
For the arrangement of compounds above, isopropanol has the highest boiling point because it forms hydrogen bonds with water. Dichloromethane possess dipole-dipole interaction which accounts for its higher boiling point. 1-butene has a higher boiling point than propane because it has higher molecular mass thus greater dispersion forces.
