Look at this system: 2A (9) mwibo C (g) + D (9) At 300K, equilibrium is...
Look at this system: 2A (9) mwilio C (g) + D (g) At 300K, equilibrium is reached, and the concentrations are found to be and to 0.0144 MA: 0.0701 M C; 0.860 MD What is Kc? O 5.05 x 10-2 O 2.91 x 103 O 0.990 O 7.06 x 102 O 0.0405 O 9.63
Look at this system: 2A (g) and C (g) + D (g) At 300K, equilibrium is reached, and the concentrations are found to be 0.0824 M A; 0.0946 MC; 0.652 MD What is Kc? 9.08 552 0.00590 3.86 x 106 0.0995 0.00345
Look at this system: 2A (9) + B (9) C (9) + D (9) At 300K, equilibrium is reached, and the concentrations are found to be 0.114 M A; 0.0701 M B; 0.246 M C 0.0352 MD What is Kc? o 9.50 o 335 0.590 o 1.24 x 10-3 e 0.139 0 245 3.05
Question 4 Look at this system: 2A (g) + B (g) 2C (g) At 300K, equilibrium is reached, and the concentrations are found to be 0.0657 MA; 0.0750 MB; 0.0256 MC What is Kc? 2.02 7.82 6.23x 105 5.24 x 10-2 5.01 x 10-1 253 723 6.73 x 10-3
quick!!!!!!
Given the reaction at 300K: 2A(g) = 3B(g) + C(g) Kc = 5.5 x 10-5. If 12.0 moles of A is added to a 3.0L container (hint, you need molarity not moles in your ICE table), what will the concentration of A be at equilibrium? Neglect x for this problem. Report your answer to 2 significant figures. Answer: 3.8
For System 2A(g) + 5 B(g) →64 C(g) + 6D (g) when reaching balance 37 degrees Celsius concentrations are: (a.) 0.110 M, (b.) 0.050 M, (c.) 0.200 M a.) what is the value of Kc? b.) what is the value of Kp?
What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=5.3 Gaseous hydrogen iodide is placed in a closed container at 425∘C, where it partially decomposes to hydrogen and iodine: 2HI(g)⇌H2(g)+I2(g) At equilibrium it is found that [HI]= 3.55×10−3M, [H2]= 4.82×10−4M , and [I2]= 4.82×10−4M. What is the value of Kc at this temperature? b The reversible...
For the Equilibrium System N2 (g) + O2 (g) === 2 NO (g) 1.) Write a Kc and a Kp expression. 2.) If Kc = 1.50 x 10-2 at 653oC, Calculate and report the equilibrium concentrations of all of the reactants and all of the products at 653oC, if the initial concentrations were [N2]0 = 0.0100 M [O2]0 = 0.0200 M [NO]0 = 0.00300 M 3.) Calculate Kp for this equilibrium system at 653oC using the equation Kp = Kc(RT)∆n....
Again, consider the exothermic reaction, with K=3.00: 2A(aq) + B(g) ⇌ C(aq) + D(g) With initial concentrations of [A] = 0.5M, [B] = 2.0M, [C] = 1.0M, and [D] = 1.5M. For each of the following disruptions, predict weather the reaction will go forward (toward products), reverse (towards reactants), or be unchanged. a) [A] increased to 2.0M b) Pressure doubled. c) Volume of solution doubled by dilution. d) The temperature is increased by 100.0oC (15.83 from text) When 1.50mol CO2...
A(g) -> B(g)+C(g) Find the equilibrium concentrations of A,
B, and C for each of the following different values of Kc. Assume
that the initial concentration of A in each case is 1.0 M and that
the reaction mixture initially contains no products.
UNITS_18_19_HW Exercise 15.61 A Review Constants 1 Peric Submit Request Answer Consider the following reaction: A(9) B(9) + C(9) Find the equilibrium concentrations of A, B, and C for each of the following different values of Ke....