Answer:
The answer is either A or C figure it out sorry
When Q is equal the initial concentration of the products / the initial concentration of the reactants.
so, Q = [Ag]*[Cl-] and we neglected [AgCl] as it is solid
∴ Q = 10^-6 * 10^-5
= 10^-11
now we will compare the value of Q with the value of Keq:
when Q = Keq so, the system is in equilibrium
and when Q > Keq so, the reaction will go forward (shift to right) to achieve equilibrium.
and when Q< Keq so, the reaction will go left (shift to left) to achieve equilibrium.
when Q = 10^-11 and Keq = 10^20
∴Q< Keq
and the reaction will shift to left.
Answer:
69.6L
Explanation:
Using Charles law equation:
V1/T1 = V2/T2
Where;
V1 = initial volume (L)
V2 = final volume (L)
T1 = initial temperature (K)
T2 = final temperature (K)
According to this question, a gas takes up 50.0 L while at STP. A gas at STP will possess an initial temperature of 273K. Hence;
V1 = 50.0 L
V2 = ?
T1 = 273K
T2 = 380K
Using V1/T1 = V2/T2
50/273 = V2/380
CROSS MULTIPLY
380 × 50 = 273 × V2
19000 = 273V2
V2 = 19000 ÷ 273
V2 = 69.59
V2 = 69.6L
