Question

Consider mixture B, which will cause the net reaction to proceed forward. Concentration (M)initial:change:equilibrium:[XY]0.500−x0.500−xnet→⇌[X]0.100+x0.100+x+[Y]0.100+x0.100+x The change...

Consider mixture B, which will cause the net reaction to proceed forward.

Concentration (M)initial:change:equilibrium:[XY]0.500−x0.500−xnet→⇌[X]0.100+x0.100+x+[Y]0.100+x0.100+x

The change in concentration, x, is negative for the reactants because they are consumed and positive for the products because they are produced.

A) Based on a Kc value of 0.210 and the given data table, what are the equilibrium concentrations of XY, X, and Y, respectively?

Express the molar concentrations numerically.

Consider mixture C, which will cause the net reaction to proceed in reverse.

Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+x←net⇌[X]0.300−x0.300−x+[Y]0.300−x0.300−x

The change in concentration, x, is positive for the reactants because they are produced and negative for the products because they are consumed.

B) Based on a Kc value of 0.210 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?

Express the molar concentrations numerically.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider mixture B, which will cause the net reaction to proceed forward. Concentration (M)initial:change:equilibrium:[XY](0.500) (−x) (0.500−x)...
Consider mixture B, which will cause the net reaction to proceed forward. Concentration (M)initial:change:equilibrium:[XY](0.500) (−x) (0.500−x) net→⇌[X](0.100) (+x) (0.100+x) +[Y](0.100) (+x) (0.100+x) The change in concentration, x, is negative for the reactants because they are consumed and positive for the products because they are produced. Part B Based on a Kc value of 0.130 and the given data table, what are the equilibrium concentrations of XY, X, and Y, respectively? Express the molar concentrations numerically. Consider mixture C, which will...
Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will cause the...
Calculating equilibrium concentrations when the net reaction proceeds forward Consider mixture B, which will cause the net reaction to proceed forward. Concentration (M)initial:change:equilibrium:[XY]0.500−x0.500−xnet→⇌[X]0.100+x0.100+x+[Y]0.100+x0.100+x The change in concentration, x, is negative for the reactants because they are consumed and positive for the products because they are produced. Part B Based on a Kc value of 0.130 and the given data table, what are the equilibrium concentrations of XY, X, and Y, respectively? Express the molar concentrations numerically. Calculating equilibrium concentrations when...
Consider mixture C, which will cause the net reaction to proceed in reverse. Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+x←net⇌[X]0.300−x0.300−x+[Y]0.300−x0.300−x The...
Consider mixture C, which will cause the net reaction to proceed in reverse. Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+x←net⇌[X]0.300−x0.300−x+[Y]0.300−x0.300−x The change in concentration, x, is positive for the reactants because they are produced and negative for the products because they are consumed.
Based on a Kc value of 0.200 and the data table given, what are the equilibrium...
Based on a Kc value of 0.200 and the data table given, what are the equilibrium concentrations of XY , X , and Y , respectively? Express the molar concentrations numerically. Consider mixture C, which will cause the net reaction to proceed in reverse. Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+x←net⇌[X]0.300−x0.300−x+[Y]0.300−x0.300−x The change in concentration, x , is positive for the reactants because they are produced and negative for the products because they are consumed.
Consider the following reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and Cfor each of...
Consider the following reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and Cfor 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. Make any appropriate simplifying assumptions. Kc= 1.2 Kc= 1.8x10−2 Kc= 2.0×10−5 Express your answer using two sig figs. Enter your answers numerically seperated by commas.
Consider the reaction for the Haber Process: 3H2 (g) + N2 (g) <--> 2NH3(g) A mixture...
Consider the reaction for the Haber Process: 3H2 (g) + N2 (g) <--> 2NH3(g) A mixture of 1.0 mol each of N2, H2, and NH3 are placed into a 1.0 L flask and allowed to come to equilibrium at 500.0 C. Kp at this temperature is 1.45 x 10-5 atm-2. A.) What is the value of Kc at this temperature? irst find the relationship between Kc and Kp in terms of RT. Then substitute T = 773K and R =...
Consider the reaction: N2(g) + 3H2(g) → 2NH3(g). At a particular moment during the reaction hydrogen...
Consider the reaction: N2(g) + 3H2(g) → 2NH3(g). At a particular moment during the reaction hydrogen is being consumed at a rate of 0.074 M/s. At this moment: (a) What is the rate of reaction (in M/s)? {3 points} (b) A what rate (in M/s) is NH3 being produced? {3 points} (c) Are these average or instantaneous rates? {1 point} [3] A certain first-order reaction has a rate constant of 1.65 min-1 at 20°C. What is the value of the...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are equal b)the value of the equilibrium constant is 1 c)all chemical reactions have ceased d)the rate constants of the forward and reverse reactions are equal e)the limiting reagent has been consumed 2)The equilibrium-constant expression depends on the ________ of the reaction. a) stoichiometry b) mechanism c) the quantities of reactants and products initially present d) temperature e) stoichiometry and mechanism 3)Given the following reaction...