Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![< PREV
NEXT >
The value of Kc is 280 at a specific temperature. Based on your ICE table (Part 1),
set up the equilibrium expression for Kc in order to determine concentrations of all
species. Each reaction participant must be represented by one tile. Do not
combine terms.
[x]
[0.133 + 2x]
[0.133 + 2x]²
Predict the equilibrium concentration of IBr in the reaction described
below by constructing an ICE table, writing an equilibrium
expression for Kc, and solving for the equilibrium concentration.
Complete Parts 1-3 before submitting your answer.
12(g) + Br₂(g) 2 IBr(g)
Tap here or pull up for additional resources
[2x]
[0.133 -x]
[0.133 - x]²
1
Kc =
Кс
[2x]²
[0.133 - 2x]
[0.133 - 2x]²
[0.400 + x]
[0.400 + x]²
[0.400 + 2x]
[0.400 + 2x]²
3
= 280
[0.400 -x]
[0.400 -x]²
[0.400 - 2x]
[0.400 - 2x]²
RESET
[0.133 + x]
[0.133 + x]²](https://content.bartleby.com/qna-images/question/21b2424c-a4ba-45d0-aa84-edf812370fbb/1934f539-8ec6-40f8-a1e9-02bdf2ed6dd3/n3981f_processed.jpeg)
Transcribed Image Text:< PREV
NEXT >
The value of Kc is 280 at a specific temperature. Based on your ICE table (Part 1),
set up the equilibrium expression for Kc in order to determine concentrations of all
species. Each reaction participant must be represented by one tile. Do not
combine terms.
[x]
[0.133 + 2x]
[0.133 + 2x]²
Predict the equilibrium concentration of IBr in the reaction described
below by constructing an ICE table, writing an equilibrium
expression for Kc, and solving for the equilibrium concentration.
Complete Parts 1-3 before submitting your answer.
12(g) + Br₂(g) 2 IBr(g)
Tap here or pull up for additional resources
[2x]
[0.133 -x]
[0.133 - x]²
1
Kc =
Кс
[2x]²
[0.133 - 2x]
[0.133 - 2x]²
[0.400 + x]
[0.400 + x]²
[0.400 + 2x]
[0.400 + 2x]²
3
= 280
[0.400 -x]
[0.400 -x]²
[0.400 - 2x]
[0.400 - 2x]²
RESET
[0.133 + x]
[0.133 + x]²
![Initial (M)
Change (M)
Equilibrium (M)
0.400 + x
Predict the equilibrium concentration of IBr in the reaction described
below by constructing an ICE table, writing an equilibrium
expression for Kc, and solving for the equilibrium concentration.
Complete Parts 1-3 before submitting your answer.
12(g) + Br₂(g) 2 IBr(g)
Tap here or pull up for additional resources
In a 3.0 L container at high temperature, 0.400 mol of IBr is allowed to reach
equilibrium. Fill in the ICE table with the appropriate value for each involved
species to determine the partial pressures of all reactants and products. Where
applicable, use the x variables to represent any unknown change in concentration.
0
1
0.400 + 2x
1₂(g)
[0]
0.400
0.400 - x
0.133
2
0.400 - 2x
+
+x
3
Br₂(g)
0.133 + x
110
+2x
0.133 + 2x
NEXT >
-X
0.133 - x
2 IBr(g)
000
RESET
-2x
0.133 - 2x](https://content.bartleby.com/qna-images/question/21b2424c-a4ba-45d0-aa84-edf812370fbb/1934f539-8ec6-40f8-a1e9-02bdf2ed6dd3/lwfwapd_processed.jpeg)
Transcribed Image Text:Initial (M)
Change (M)
Equilibrium (M)
0.400 + x
Predict the equilibrium concentration of IBr in the reaction described
below by constructing an ICE table, writing an equilibrium
expression for Kc, and solving for the equilibrium concentration.
Complete Parts 1-3 before submitting your answer.
12(g) + Br₂(g) 2 IBr(g)
Tap here or pull up for additional resources
In a 3.0 L container at high temperature, 0.400 mol of IBr is allowed to reach
equilibrium. Fill in the ICE table with the appropriate value for each involved
species to determine the partial pressures of all reactants and products. Where
applicable, use the x variables to represent any unknown change in concentration.
0
1
0.400 + 2x
1₂(g)
[0]
0.400
0.400 - x
0.133
2
0.400 - 2x
+
+x
3
Br₂(g)
0.133 + x
110
+2x
0.133 + 2x
NEXT >
-X
0.133 - x
2 IBr(g)
000
RESET
-2x
0.133 - 2x
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- A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g) C₂H₂(g) + 3H₂(g) K₁=3. × 10 P -6 He fills a reaction vessel at this temperature with 6.0 atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of C₂H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of C₂H₂ at right. Round your answer to 1 significant digit. 0 yes no atm x10 X Śarrow_forwardO KINETICS AND EQUILIBRIUM Try again. 2/5 Calculating equilibrium composition from an equilibrium constant Try Again Suppose a 500. mL flask is filled with 1.5 mol of O, and 0.60 mol of NO. The following reaction becomes possible: N,(g) +0,(2) – 2No(2) The equilibrium constant K for this reaction is 5.01 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places. 3.36 M IIarrow_forwardAt a certain temperature, the reaction: PCl5(g) ⇆ PCl3(g) + Cl2(g) has an equilibrium constant Kc = 6.7E-6. Calculate the equilibrium concentration of PCl3 if only PCl5 is present initially at a concentration of 0.30 M. Your answer should have two significant figures.arrow_forward
- Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after a decrease in pressure or volume. If there is no change in the concentration of the species, leave the box blank. CH, (g) + 2 H, S(g) = CS, (g) + 4 H, (g) after decreasing the pressure after decreasing the volume of the reaction vessel Answer Bankarrow_forwardAt equilibrium, the concentrations in this system were found to be [N,] = [0,] = 0.100 M and [NO] = 0.400 M. N, (g) + 0,(g) = 2 NO(g) If more NO is added, bringing its concentration to 0.700 M, what will the final concentration of NO be after equilibrium is re-established? [NO]final = Marrow_forwardFor the reaction 2 NO(g) + Cl2 (g) *double arrow here* 2 NOCl (g) at 25 ℃, the equilibrium constant is 10.0. If at equilibrium, [NOCl] = 2.6 M, [NO] = 0.34 M, what is the concentration of chlorine gas?arrow_forward
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