1. An equimolar mixture of hydrogen and iodine was heated at 400°C no until further change inthe concentration of H2, l2, or HI was observed. At this point it was assumed that equilibriumhad been reached, and it was found by analysis that [H2] = 0.221 M, [12] = 0.221 M, and [HI] =1.563 M. Calculate the equilibrium constant for the reaction at 400°C.H2(g) + I2(g)2HI(g)2. If 60.0 g each of acetic acid (CH;CO2H) and ethanol (C2H;OH) are allowed to react in a 1.00-Lsealed container until equilibrium is established, how many moles of the ester (CH3CO2C;Hs)andwater are formed, and how many moles of ethanol and acid remain?(K = 4.00.)CH3CO2H + C2H5OHCH;CO2C2H5 + H20

Please note- As per our company guidelines we are supposed to answer only one question. Kindly…

1. An equimolar mixture of hydrogen and iodine was heated at 400°C no until further change in the concentration of H2, I2, or HI was observed. At this point it was assumed that equilibrium had been reached, and it was found by analysis that [H2] = 0.221 M, [l2] = 0.221 M, and [HI] = 1.563 M. Calculate the equilibrium constant for the reaction at 400°c. H2(8) + Iz(8) 2HI(g)

1. An equimolar mixture of hydrogen and iodine was heated at 400°C no until further change in the concentration of H2, I2, or HI was observed. At this point it was assumed that equilibrium had been reached, and it was found by analysis that [H2] = 0.221 M, [l2] = 0.221 M, and [HI] = 1.563 M. Calculate the equilibrium constant for the reaction at 400°c. H2(8) + Iz(8) 2HI(g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: The equilibrium constant, K., for the following reaction is 1.47 at 665 K. 2NH3(g) N2(g)+ 3H2(g)…

A: 2NH3 (g) ----> N2 (g) + 3H2 (g) initial a 0…

Q: 2. (a) MeO Least basic List the following compounds in order of increasing basicity. NH₂ NH₂ NH (N-J…

Q: A mixture initially contains A, B, and C in the following concentrations: [A] = 0.450 M , [B] = 1.00…

Q: The following reaction was performed in a sealed vessel at 771 °C : H2 (g) + I2(g) = 2HI(g)…

Q: The equilibrium constant Kp= (5.1 x 10^-2) for the following reaction in gas phase at a given…

A: We will first write Kp expression, then using ICE table calculate equilibrium concentrations of…

Q: Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated…

Q: The equilibrium constant, Ke, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g)=2 HI (g)…

A: Note : Dear student as per guidelines one question is allowed to solve, thank you please post is…

Q: Assume that the reaction for the formation of gaseous hydrogen fluoride from gaseous hydrogen and…

A: Balance chemical equation: H2 (g) + F2 (g) ⇌…

Q: The equilibrium constant, K., for the following reaction is 9.52×10-2 at 350 K. CH (g) + CCl, (g)=2…

Q: Predict v ianges in the compositions the engineer should expect next time he measures the…

Q: Iodine and bromine react to give iodine monobromide, IBr. 4(9) + Br3 (9) = 2IBr(9) What is the…

Q: Suppose a 500, mil. flask is filled with 1.8 mol of OCI, 1.0 mol of BrOCI and 1.4 mol of BrCl. The…

Q: A chemical engineer is studying the following reaction: CH (9)+2H,S(9) CS,(9)+4H,(9) At the…

A: Answer:- This question is answered by using the simple concept of reaction quotient and equilibrium…

Q: • In an analysis of inter halogen reactivity, 0.500 mol ICI (iodine chloride) was placed in a 5.00 L…

Q: The equilibrium constant Kp = (8.71x10^-1) for the following reaction in the gas phase at a given…

A: Given,

Q: equilibrium constant: aA(g) bB (g), K = 2.2 Part B Find the equilibrium concentrations of A and B…

Q: The equilibrium constant at 350 K for the reaction Br2(g) + I2(g) = 2 IBr(g) has a value of 322.…

Q: A student ran the following reaction in the laboratory at 531 K: PC13 (g) + Cl₂ (9) ⇒ PC15 (9) When…

A: Using the concentration terms at equilibrium, the equilibrium constant, Kc can be calculated.

Q: Bromine monochloride is synthesized using the reaction Br₂(g) + Cl₂(g) = 2 BrCl(g) Kp = 1.1 x 10 at…

A: We have to calculate the mass of BrCl and percent yield

Q: Ammonia and oxygen react to form nitrogen and water, like this: 4NH, (g)+30,(g) 2N, (g)+6H,0(g)…

A: According to Le chatelier principle, equilibrium will shift in such way that counteracted upon…

Q: Assume that the reaction for the formation of gaseous hydrogen fluoride from gaseous hydrogen and…

A: The equilibrium reaction for formation of hydrogen fluoride is as follows: H2(g) + F2(g) ⇌ 2HF(g)…

Q: tl e tl a

A: Given the equation of the calibration curve, Y = 0.035x + 0.0148, and the absorbance values,…

Q: A chemical engineer is studying the following reaction: HCN(aq)+NH3(aq) → CN¯(aq)+NH (aq) At the…

A: The direction of the reaction depends on the reaction quotient of the reaction 1) If reaction…

Q: A student ran the following reaction in the laboratory at 691 K: 2HI(g) =H₂(g) + I₂(g) When she…

A: The given reaction is 2HI(g) ⇔H2(g) +I2(g)

Q: perature the engineer picks, the equilibrium constant K, for this reaction is 0.047. er charges…

Q: A chemical engineer is studying the following reaction: HCH,CO,(aq)+CH,NH,(aq) →…

A: For the reaction given above, CH3COOH (aq) + CH3NH2 (aq) →CH3COO- (aq) + CH3NH3+(aq) We know that,…

Q: 2NOBr(g) 2NO(g When she introduce 0.112 atm. Calculate the equilib Kp =

Q: The equilibrium constant Kp= 8.70x10^-1 for the following reaction in the gas phase at a given…

A: Pressure of H2O and Cl2O are given equal to 0.386 bar for each. Kp = 0.870

Q: Consider the equilibrium system described by the chemical reaction below. If the partial pressures…

Q: Consider the reaction and associated equilibrium constant: aA(g) bB (g), K = 2.2 Find the…

Q: The equilibrium constant, Kc, for the following reaction is 32.4 at 298 K. 2CH2CI2(g) =CH4(g) +…

Q: In an experiment conducted at 300 0C, the equilibrium concentrations of the species involved in the…

A: The given reaction is : 2NH3(g) ⇌ N2(g) + 3H2(g) at 300°C The equilibrium…

Q: reaction, I2(s) + Br2(g) ⇋ 2 IBr(g) is 0.25 at 25 °C. (a) Calculate ΔrG⦵ for this reaction. (b)…

A: Given , I2 (S) + Br2 (g) <-----> 2IBr (g) Kc = 0.25 We have to determine ∆°rG and p(IBr)…

Q: At 850 K, the equilibrium constant for the reaction 2 SO₂(g) + O₂(g) = 2 SO3(g) is Kc = 15. If the…

A: The equilibrium reaction given is 2 SO2 (g) + O2 (g) ⇌2 SO3 (g), Kc = 15 at 850 K Kc is the…

Question

1. An equimolar mixture of hydrogen and iodine was heated at 400°C no until further change in
the concentration of H2, l2, or HI was observed. At this point it was assumed that equilibrium
had been reached, and it was found by analysis that [H2] = 0.221 M, [12] = 0.221 M, and [HI] =
1.563 M. Calculate the equilibrium constant for the reaction at 400°C.
H2(g) + I2(g)
2HI(g)
2. If 60.0 g each of acetic acid (CH;CO2H) and ethanol (C2H;OH) are allowed to react in a 1.00-L
sealed container until equilibrium is established, how many moles of the ester (CH3CO2C;Hs)and
water are formed, and how many moles of ethanol and acid remain?
(K = 4.00.)
CH3CO2H + C2H5OH
CH;CO2C2H5 + H20

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Final answer

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N₂04(9) =2 NO₂(g) Three experiments were run starting with different initial amounts of N₂O4(g) ([N₂O4lo in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO₂ and N₂O4 at equilibrium. Be sure to round to the correct number of significant figures. Exp [N₂04]0 [NO₂] [N₂04] 1 3.8 2.98 2.3 2 3.1 2.64 1.8 3 2.1 2.06 1.1 [NO₂] 2 [NO₂] [NO₂]²/ [N₂04] / [N₂04] [N₂04] Based on your calculations, indicate whether each statement is True (T) or False (F): 1. Each experiment started with a different initial concentration of N₂04 2. The ratio ([NO₂] / [N₂O4]) is equal to a constant value. 3. The ratio (2…
The equilibrium constant for the reaction 2 KAl(OH)4(aq) + 4 H2SO4(aq) ⇆ 2 KAl(SO4)2(s) + 8 H2O(l) at room temperature is 84.5. At equilibrium, the concentration of sulfuric acid (H2SO4) is 0.531M. What is the concentration of KAl(OH)4 (in moles/L)?
The equilibrium constant, K, for the following reaction is 5.00x10-2 at 642 K. COCI2(g) : =CO(g) + Cl2(g) An equilibrium mixture of the three gases in a 5.49 L container at 642 K contains 0.288 M COCI2, 0.120 M CO and 0.120 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 11.9 L? [COCI2] = [CO] [Cl2] M ΣΣΣ Il||
At 850 K, the equilibrium constant for the reaction 2SO2(g) + O2(g) 2SO3(g) is K = 15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium. Left [SO₂] = 0.22 M [02] = 0.10 M [SO3] = 0.50 M [SO₂] = 0.20 M [02] = 0.60 M [SO3] = 0.60 M [SO₂] = 0.90 M [02] = 0.80 M [SO3] = 0.15 M No net reaction Answer Bank Right Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry Publish
At 850 K, the equilibrium constant for the reaction 2 SO₂(g) + O₂(g) = 2SO3(g) is Kc = 15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium. [SO₂] = 0.60 M [0₂] = 0.60 M [SO3] = = 0.13 M Left [SO₂] = 0.11 M [0₂] = 0.20 M [SO3] = 0.40 M No net reaction [SO₂2] = 0.20 M [0₂] = 0.60 M [SO3] = 0.60 M Answer Bank Right
The equilibrium constant, K, for the following reaction is 1.80x104 at 298 K. NH,HS(s)=NH3(g)+ H2S(g) Calculate the equilibrium concentration of H2S when 0.221 moles of NH,HS(s) are introduced into a 1.00 L vessel at 298 K.
At 286 K and a total equilibrium pressure of 0.972 atm, the fractional dissociation of NO is 0.276 for the reaction 2NO(g) N₂(g) + O₂(g) This means that 276 of every 1000 molecules of NO originally present have dissociated. Calculate the equilibrium constant in terms of pressures, Kp. Kp
1 A + 2 B → 2 C Calculate the equilibrium constant (K) for the following reaction at 1000. K, using this information: A and B are placed in a flask and at the beginning of the reaction [A] is 8.95 M and [B] is 6.21 M. After the reaction has reached equilibrium,[B] is 1.94 M. Please ignore significant figures for this problem.
3) Calculate the equilibrium concentrations of H2, I2 and HI at 700.K if the initial concentrations are [H2] = 0.200M, [I2] = 0.200M. The equilibrium constant Kc for the reaction is 57.0 at 700K.
Expectation: investigate the qualitative and quantitative nature of chemical systems at equilibrium, and solve related problems.
An experimenter places the following concentrations of gases in a closed container: NOB1] = 0.475 M, [NO] = 2.59 x 10-2 M, Bra] = 5.57 x 10-2 M. These gases then react: 2NOB1(g) = 2NO(g) + Br2 (g) At the temperature of the reaction, the equilibrium constant Ke is 3.15 x 10-4. Calculate the reaction quotient, Qe, from the initial concentrations and determine whether the concentration of NOBr increases or decreases as the reaction approaches equilibrium. Qc = The concentration of NOBr decreases v
Initially, 1.50 M of ammonia (NH3) were placed in an empty container without any other gases at 789K. It started to decompose according to the chemical equation below: 2 NH3(g) = N₂(g) + 3 H₂(g) After equilibrium was established, it was found that there are 0.055 M of ammonia left in the same vessel. What is the equilibrium constant, Kc, for this reaction at 789 K? 3.5 28 9.8 x 103 2.4 x 10³ O4.8 x 104