The full question is shown in the image attached to this answer
Answer:
6.2 * 10^-3
Explanation:
The reaction at equilibrium is as follows;
TiCl4(l) → Ti(s)+ 2Cl2(g)
We have to obtain the concentration of chlorine gas as follows;
[Cl2] = 1.08/70.91 g/mol × 5.2 L
[Cl2] = 0.079 M
Kc = [Cl2]^2
Kc = [ 0.079]^2
Kc = 6.2 * 10^-3
Answer:
The partial pressure of argon in the flask = 71.326 K pa
Explanation:
Volume off the flask = 0.001
Mass of the gas = 1.15 gm = 0.00115 kg
Temperature = 25 ° c = 298 K
Gas constant for Argon R = 208.13
From ideal gas equation P V = m RT
⇒ P =
Put all the values in above formula we get
⇒ P = × 208.13 × 298
⇒ P = 71.326 K pa
Therefore, the partial pressure of argon in the flask = 71.326 K pa