Consider the following equilibrium at 25.0 degrees C and the information about initial concentrations, and answer...
Consider the following equilibrium at 25.0 degrees C and the
information about initial concentrations, and answer the
question:
CH4(g) + 2H2S
(g)
CS2(g)
+ 4H2(g)
In one experiment, 4.00 M CH4, 4.00 M
CS2, 8.00 M H2S and 8.00 M
H2 in a 1.00 L vessel at 1000 degrees C. Kc is
0.036.
After the system is allowed to reach equilibrium, which of the
following concentrations for H
2 and H 2S are
reasonable, given the above initial concentrations? (Only one set
of values is reasonable). Hint: you have to solve for Q and decide
if the reaction will go right or left; that is all you have to
do--it isn’t harder than that.
|
H 2S = 3.66 M; H 2 = 13.8 M |
||
|
H 2S = 11.12 M ; H 2 = 1.76 M |
||
|
H 2S = 0.529 M; H 2 = 10.4 M |
||
|
H 2S = 6.35 M; H 2 = 8.50 M |
||
|
H 2S = 7.28 M; 15.9 M |
Homework Answers
![..CHu cos + p Hy sces 3 csopce, + 49 cm f 4 HI 4M 4M 8M Qc fun= xn 64 (4) Cype [csg] [ Ho JS (4) C894 64 [CH] [ Hos 3 por ac](http://img.homeworklib.com/questions/33163ea0-db58-11eb-8057-7125c9fbe58f.png?x-oss-process=image/resize,w_560)
Add Answer to:
Consider the following equilibrium at 25.0 degrees C and the
information about initial concentrations, and answer...
For the equilibrium, CH4(g) + 2 H2S(g) = CS2(g) + 4H2(g), the concentrations at equilibrium are...
For the equilibrium, CH4(g) + 2 H2S(g) = CS2(g) + 4H2(g), the concentrations at equilibrium are (CH4) = 0.3322 M, [H2S] = 0.6644 M, [CS2] = 0.0678 M, and [H2] = 0.2712 Mat 1400.0 K. Calculate K. O 0.167 2.50 x 10-3 C) 4.00 - 103
Suppose a 250. mL flask is filled with 1.7 mol of H2S, 2.0 mol of CS2...
Suppose a 250. mL flask is filled with 1.7 mol of H2S, 2.0 mol of CS2 and 0.50 mol of H 2. This reaction becomes possible: CH_(8) +2H2S(g) = CS2(g) + 4H2 () Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change...
Consider the following equilibrium and the information about initial concentrations, and answer two questions: Cl2(g) +...
Consider the following equilibrium and the information about initial concentrations, and answer two questions: Cl2(g) + F2 (g) 2CIF (9) In one experiment, 0.0600 mol Cl2 and 0.0600 mol F2 are placed in a 2.00 L vessel at a certain temp. Kc at this temp is 19.8. What is concentration of Cl2 at equilibrium? Hint--don't need quadratic HINT: you need to divide the moles by 2.00 L to find the molarities 0.00930 M o 2.00 x 10-4 M. 1.92 x...
Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition...
Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition of nitrogen monoxide. 2NO(g) N2(g) + O2(g) [N2] [02] K=— = 3.62x10-2 at 286 K [NO] A flask originally contains 0.239 M nitrogen monoxide. Calculate the equilibrium concentrations of the three gases. [NO] = [N2] = [02] =
Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition...
Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition of hydrogen iodide. 2HIG) P H2(g) +12(g) [H2] [12] K=— =1.98x10-2 at 895 K (HI) A flask originally contains 0.373 M hydrogen iodide. Calculate the equilibrium concentrations of the three gases. [HI] = [H2) = [12] =
The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] =...
The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] = 0.275 M , [H2] =0.300 M , and [S2] = 0.00 M. Find the equilibrium concentration of [S2].
The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] =...
The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] = 0.175 M , [H2] =0.350 M , and [S2] = 0.00 M. Find the equilibrium concentration of [S2].
The reaction 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7, at 800∘C is carried out with the following initial concentrations: [H2S] =...
The reaction 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7, at 800∘C is carried out with the following initial concentrations: [H2S] = 0.375 M , [H2] =0.125 M , and [S2] = 0.000 M. Find the equilibrium [S2]. Express your answer with the appropriate units.
Question 25 1) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature....
Question 25 1) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g) (3 marks) CH4(g) + H2O(g) = C,H,OH(g) ke -9.0 * 10 M [CH]eq=0.015 mol CH2OHjeq = 1.69 moll A) 9.9 x 10 mol L' B) 80. mol L' C) 1.0 mol L. D) 1.68 mol L' E) 0.013 mol L'
1) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.590; [SCN-]...
1) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.590; [SCN-] = 1.239; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.454 M. What is the numerical value of KC for this equilibrium? KC = __________________ 2) Consider the following equilibrium: Fe3+(aq) + SCN-(aq) ⇌ FeSCN2+(aq) Initial concentrations: [Fe3+] = 0.370; [SCN-] = 0.777; [FeSCN2+] = 0 The equilibrium concentration of [FeSCN2+]eq = 0.285 M. What is the equilibrium concentration of Fe3+? [Fe3+]eq =...
For the equilibrium, CH4(g) + 2 H2S(g) = CS2(g) + 4H2(g), the concentrations at equilibrium are (CH4) = 0.3322 M, [H2S] = 0.6644 M, [CS2] = 0.0678 M, and [H2] = 0.2712 Mat 1400.0 K. Calculate K. O 0.167 2.50 x 10-3 C) 4.00 - 103
Suppose a 250. mL flask is filled with 1.7 mol of H2S, 2.0 mol of CS2 and 0.50 mol of H 2. This reaction becomes possible: CH_(8) +2H2S(g) = CS2(g) + 4H2 () Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change...
Consider the following equilibrium and the information about initial concentrations, and answer two questions: Cl2(g) + F2 (g) 2CIF (9) In one experiment, 0.0600 mol Cl2 and 0.0600 mol F2 are placed in a 2.00 L vessel at a certain temp. Kc at this temp is 19.8. What is concentration of Cl2 at equilibrium? Hint--don't need quadratic HINT: you need to divide the moles by 2.00 L to find the molarities 0.00930 M o 2.00 x 10-4 M. 1.92 x...
Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition of nitrogen monoxide. 2NO(g) N2(g) + O2(g) [N2] [02] K=— = 3.62x10-2 at 286 K [NO] A flask originally contains 0.239 M nitrogen monoxide. Calculate the equilibrium concentrations of the three gases. [NO] = [N2] = [02] =
Use K and initial concentrations to calculate equilibrium concentrations. Consider the equilibrium system involving the decomposition of hydrogen iodide. 2HIG) P H2(g) +12(g) [H2] [12] K=— =1.98x10-2 at 895 K (HI) A flask originally contains 0.373 M hydrogen iodide. Calculate the equilibrium concentrations of the three gases. [HI] = [H2) = [12] =
Question 25 1) Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g) (3 marks) CH4(g) + H2O(g) = C,H,OH(g) ke -9.0 * 10 M [CH]eq=0.015 mol CH2OHjeq = 1.69 moll A) 9.9 x 10 mol L' B) 80. mol L' C) 1.0 mol L. D) 1.68 mol L' E) 0.013 mol L'
Most questions answered within 3 hours.
-
In 2003, an organization surveyed 1 comma 510 adult Americans
and asked about a certain war,...
asked 5 minutes ago -
Blue colorin fireworks is often achieved by heating copper(I)
chloride (CuCl) to about 1200°C. Then the...
asked 10 seconds from now -
Coperto Insurers of Davenport, Iowa offers four different
insurance plans, all of which are equally popular...
asked 7 minutes ago -
A 50 mL graduated cylinder contains 25.0 mL of water. A 42.5040
g piece of gold...
asked 9 minutes ago -
Leo’s Lamp Store sells table and floor lamps. For a floor lamp,
the holding cost is...
asked 11 minutes ago -
Mark Gershon, owner of a musical instrument distributorship,
thinks that demand for guitars may be related...
asked 22 minutes ago -
Suppose that you were asked to construct a 95% confidence
interval based on the standard normal...
asked 30 minutes ago -
3 - What decimal number does the bit pattern 11001100 represent
if it is a:
•...
asked 32 minutes ago -
The copper(II) ion is acidic whereas the acetate ion is basic.
However, copper acetate is acidic....
asked 28 minutes ago -
A 48.53 mL volume of 1.00 M HCl was mixed with 47.70 mL of 2.00
M...
asked 50 minutes ago -
Neural cell types can be specified from ESCs with
retinoic acid, conditioned medium, co-cultures or by...
asked 54 minutes ago -
Can anyone solve: "Simulation with Arena 6th Edition - Chapter 8
- Question 3E"
8-3 Change...
asked 51 minutes ago