To determine the number of gas particles in the vessel we add all of the components of the gas. For this, we need to convert the mass to moles by the molar mass. Then, from moles to molecules by the avogadro's number.
1.50x10^-6 ( 1 / 28.01) (6.022x10^23) = 3.22x10^16 molecules CO
6.80x10^-6 ( 1 / 2.02) (6.022x10^23) = 2.03x10 18 molecules H2
Totol gas particles = 2.05x10^18 molecules
Answer:
P = 17.9618 atm
Explanation:
The osmotic pressure can be calculated and treated as if we are talking about an ideal gas, and it's expression is the same:
pV = nRT
However the difference, is that instead of using moles, it use concentration so:
p = nRT/V ----> but M = n/V so
p = MRT
We have the temperature of 18 °C (K = 18+273.15 = 291.15 K) the value of R = 0.08206 L atm / K mol, so we need to calculate the concentration, and we have the mass of HCl, so we use the molar mass of HCl which is 36.45 g/mol:
n = 13.7/36.45 = 0.3759 moles
M = 0.3759/0.5 = 0.7518 M
Now that we have the concentration, let's solve for the osmotic pressure:
p = 0.7518 * 0.08206 * 291.15
<em><u>p = 17.9618 atm</u></em>
Answer:
k = 1.3 x 10⁻³ s⁻¹
Explanation:
For a first order reaction the integrated rate law is
Ln [A]t/[A]₀ = - kt
where [A] are the concentrations of acetaldehyde in this case, t is the time and k is the rate constant.
We are given the half life for the concentration of acetaldehyde to fall to one half its original value, thus
Ln [A]t/[A]₀ = Ln 1/2[A]₀/[A]₀= Ln 1/2 = - kt
- 0.693 = - k(530s) ⇒ k = 1.3 x 10⁻³ s⁻¹
5-10 seconds xxx :) hope this helps
