the question is " 3A + 2B --><--4C with Kc=1.73x10^23, if at this temperature 1.00 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?" this is my work so far, I am not sure how to go further.
the question is " 3A + 2B --><--4C with Kc=1.73x10^23, if at this temperature 1.00 mol...
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. 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, 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, 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. 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, Kc 3 A(g) 2 B(g)= 4C(g) = 1.53 x 1019 К If, at this temperature, 2.10 mol of A and 3.80 mol of B are placed in a 1.00L container, what are the concentrations of A, B, and C at equilibrium? [A] М М [B= [C] М =
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)-
the hints say use a reverse reaction and find the concentration of A. i did this. and i dint know how to go furthur At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Ke 3 A(g) + 2B() 4C(g) K -1.33 x 1015 If, at this temperature, 1.30 mol of A and 3.80 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? (A)...
4. (10 Pts) A 1.00-L flask was filled with 2.00 mol gaseous SO, and 2.00 mol gaseous NO, and heated. After equilibrium was reached, it was found that 1.30 mol gaseous NO was present. Assume that the reaction: SO2(g) + NO2(g) =SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant, Kc. 5. (12 Pts) At a particular temperature, Kc = 1.00 x 10 for the reaction H2(g) + 12(g) = 2 HI(g) In an experiment,...
Question 10 of 23 > At a certain temperature, 0.4011 mol of N2 and 1.641 mol of H2 are placed in a 4.00 L container N2(g)+3 H2 g) 2NH3(g) At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, Ke