Question

A 10.0 L container contains 1.0 L of solution of a gas. Assume [gas] = 1.5...

A 10.0 L container contains 1.0 L of solution of a gas. Assume [gas] = 1.5 x 10^-4 M in solution when 2 mol of gas remains in gas form. If 1 mol of gas is removed from the gas phase, what will be the new concentration of the gas in the solution? What is the value of k? c = kP

Homework Answers

Answer #1

In case of dissolution of gas in liquid Gas Gas in solution

Equilibrium Constant (Kc) = [Gas]/[Gas in solution]

[Gas in solution] = 1.5 x 10-4 M

  [Gas] = 2/9 (2 mole of gas occupies remaining 9 L of empty space of the container)

= 2.2 x 10-1 M

Kc   = (1.5 x 10-4 M)/(2.2 x 10-1 M)

= 6.8 x 10-4

[Gas] after removal of 1 mole of Gas from container = 1/9

= 1.1 x 10-1 M

[Gas in solution] after removal of 1 mole of Gas from container = Kc x [Gas]

= (6.8 x 10-4) x (1.1 x 10-1 M)

= 7.5 x 10-5 M

In this case concentration of the gas is praportional to the pressure of the gas

Kc = Kp

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
Calculate the pH of a 1 L solution that contains 1.0 M HCl and 1.5 M...
Calculate the pH of a 1 L solution that contains 1.0 M HCl and 1.5 M CH3COOK. The Ka for CH3COOH is 1.8 x 10-5
Calculate the pH of a 1 L solution that contains 1.0 M HCl and 1.5 M...
Calculate the pH of a 1 L solution that contains 1.0 M HCl and 1.5 M CH3COOK. The Ka for CH3COOH is 1.8 x 10-5. 9.56                             b) 4.74                         c) 4.44                        d) 0.30                         e) 7.45
A 1 liter solution of diluted liquid chloroform with toluene is in a sealed container. The...
A 1 liter solution of diluted liquid chloroform with toluene is in a sealed container. The mole fraction of chloroform in the gas phase was measured at 1500 ppmv once the solution was prepared. The molecular weight is 119.35 g/mol for chloroform and 92.13 g/mol for toluene. The vapor pressure of chloroform and toluene are 151 mmHg and 28.1 mmHg, respectively. What must the volume of liquid chloroform be in order to make a 1.0 liter total volume solution? What...
A gas-phase decomposition is first-order with respect to the reactant, R. If the initial concentration of...
A gas-phase decomposition is first-order with respect to the reactant, R. If the initial concentration of R is 1.0 ´ 10-4 mol L-1 and the rate constant k = 1.08 ´ 10-6 s-1, what concentration of R remains after 25 days? *show all work, explanations, and calculations
If 10.0 mL of 1.0 M HBr is added to 1.00 L of the solution in...
If 10.0 mL of 1.0 M HBr is added to 1.00 L of the solution in question 3, what is the resulting solution’s pH? Question 3 and results**** What is the pH of a solution with a HBrO concentration of 0.10 M and a NaBrO concentration of 0.20 M? Br2(l) + H2O(l) ↔ HOBr(aq) + HBr (aq) HOBr(l) + NaOH(l) ↔ NaOBr(aq) + H2O (aq) by using hendersen-hasselbalch equation we get, pK = pH + log {[conj.base]/[conj.acid]} {by standard we...
A and B form an ideal solution at 298 K, with xA(l)=0.55, P*A = 0.1296 atm...
A and B form an ideal solution at 298 K, with xA(l)=0.55, P*A = 0.1296 atm and P*B = 0.0758 atm. a. Calculate the partial pressures of A and B in the gas phase. b. A portion of the gas phase is removed and condensed in a separate container. Calculate the partial pressures of A and B in equilibrium with this liquid sample at 298 K.
A 1.0 L buffer solution contains 0.192 MHC2H3O2 and 0.192 M NaC2H3O2. The value of Ka...
A 1.0 L buffer solution contains 0.192 MHC2H3O2 and 0.192 M NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5. Because the initial amounts of acid and conjugate base are equal, the pH of the buffer is equal to pKa=−log(1.8×10−5)=4.74. Calculate the new pH after adding 0.019 mol of solid NaOH to the buffer.
A mixture of water and graphite is heated to 890 K in a 10.0-L container. When...
A mixture of water and graphite is heated to 890 K in a 10.0-L container. When the system comes to equilibrium it contains 0.895 mol each of H2 and CO and 0.302 mol of H2O and some graphite. Some O2 is added to the system and a spark is applied so that the H2 reacts completely with the O2, forming H2O. Find the amount of CO in the flask when the system returns to equilibrium.
A 1.0 L solution contains 3.00×10-4 M Cu(NO3)2 and 1.63×10-3 M ethylenediamine (en). The Kf for...
A 1.0 L solution contains 3.00×10-4 M Cu(NO3)2 and 1.63×10-3 M ethylenediamine (en). The Kf for Cu(en)22+ is 1.00×1020. What is the concentration of Cu2+(aq ) in the solution?
Consider the following reaction at equilibrium: 2H2(g)+S2(g)⇌2H2S(g)+heat In a 10.0-L container, an equilibrium mixture contains 2.20...
Consider the following reaction at equilibrium: 2H2(g)+S2(g)⇌2H2S(g)+heat In a 10.0-L container, an equilibrium mixture contains 2.20 g of H2, 10.9 g of S2 and 68.1 g of H2S. Part A What is the numerical Kc value for this equilibrium mixture? Part B If more H2 is added to the equlibrium mixture, how will the equilibrium shift? Part C How will the equilibrium shift if the mixture is placed in a 5.00-L container with no change in temperature? Part D If...