For reaction at t = 0 starting moles are given
And at t= t(equilibrium) some mole of C is formed from A&B
3A + 2 B -> 4C
at t=0 2.10 mol 3.80 mol 0.00 mol
at t= t(eq) 2.10 - 3x mol 3.80- 2x mol 4x mol
We have at equilibrium
Kc= [C] 4/( [A]3 [B]2)
And also Kc= 1.53 ×10 19
As kc is quite high we can take reaction as complete
And solve it by finding limiting reagent
Which here is A .
As A is cosumed fully.
[A] =0
2.10 - 3x= 0
x = 0.7
Now [B] = 3.80 - 2 ×0.7 = 2.40 mol/ L
Now [C] = 4 x = 4 × 0.7 = 2.80 mol/L
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc 3...
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3 A(g) + 2 B(g) = 4C(g) Kc = 2.93 x 1015 If, at this temperature, 1.40 mol of A and 3.90 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A] = 0 B) = 1.8667 [C] = | 2.967
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3 A(g) + 2B(g) = 4C(g) K. = 2.93 x 1017 If, at this temperature, 1.70 mol of A and 3.90 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A] = { [B] = [C] =
At a certain temperature, this reaction establishes an
equilibrium with the given equilibrium constant, Kc
= 3.13 x 1027
3A(g) + 2B(g)
4C(g)
If, at this temperature, 1.40 mol of A and 4.00 mol of B are
placed in a 1.00 L container, what are the concentrations of A, B,
and C at equilibrium?
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant Kc. 3A + 2B -><- 4C kc=3.13x10^29 If at this temperature, 2.50 mol of A and 3.70 mol of B are placed in a 1.00L container, what are the concentrations of A, B, C at equilibrium? I know the answer to B and C but system is keep telling me A is wrong The answer I have is [A]=0 <--- wrong [B]=2.033 <--- correct [C}=3.333 <----...
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Ke. 근 4C(g) 23 3A(g)+2B(g) K= 1.53x 10 If, at this temperature, 1.30 mol of A and 4.00 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium? Number Number Number
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, If, at this temperature, 1.50 mol of A and 4.00 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium?
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Ke! 3A(g) +2B(g) = 40() K.=2.13 10" Wat this temperature, 1.90 mol of A and 3.60 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium? Number (A)- O M Number Number (c)-
At a certain temperature, this reaction establishes an equillbrkum with the given equililbrium constant, Ke K, 2.13 x 10 If, at this temperature, 1.20 mol of A and 3.70 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium? Number Number [B Number MI
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) +12(g) = 2 HI(g) Kc = 53.3 At this temperature, 0.500 mol H, and 0.500 moll, were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI] =
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H,(g) +1,(g) = 2 HI(g) K. = 53.3 At this temperature, 0.300 mol H, and 0.300 mol I, were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI] =