HomeworkLib
Question

3a. Determine the equilibrium pressures of all the reactants and products for the equilibrium described below...

3a. Determine the equilibrium pressures of all the reactants and products for the equilibrium described below if you start with an initial pressure of carbon dioxide and carbon tetrafluoride each at 0.750 atm with no COF2 present. You can assume that the temperature is constant at 1550K.    (12 points)
2COF2(g) CF4(g)    +     CO2(g)     KP = 0.168 at 1550K
Initial pressures: PCO2 = PCF4 = 0.750 atm; PCOF2 = 0.000 atm
3b. What is the value of KC for this reaction? (2 points)
3c. If the volume was reduced by a factor of 2 (from 2000 mL to 1000 mL) what would be the partial pressure of CF4 expected after this mixture has come back to equilibrium? (4 points)

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
3a. Determine the equilibrium pressures of all the reactants and products for the equilibrium described below...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • 1. For the reaction 2A(g)⇌B(g)+2C(g), a reaction vessel initially contains only A at a pressure of...

    1. For the reaction 2A(g)⇌B(g)+2C(g), a reaction vessel initially contains only A at a pressure of PA=265 mmHg. At equilibrium, PA=41 mmHg. Calculate the value of Kp. (Assume no changes in volume or temperature.) 2. consider the following reaction: A(g)⇌2B(g) Find the equilibrium partial pressures of A and B for each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A...

  • The initial concentrations or pressures of reactants and products are given for each of the following...

    The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (d) 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) KP = 16.5; initial pressures: SO3 = 1.00 atm, SO2 = 1.00 atm, O2 = 1.00 atm (e) 2NO(g) + Cl2 (g) ⇌ 2NOCl(g) Kc = 4.6 × 104 ; [NO] = 1.00 M, [Cl2] = 1.00...

  • please explain, thanks 1a. The equilibrium for the formation of HOCl in the gas phase from...

    please explain, thanks 1a. The equilibrium for the formation of HOCl in the gas phase from chlorine dioxide (C120) is given below. What are the expected equilibrium pressures if a cylinder has initial pressures as follows: PC120 = PH20 = 0.45 atm; Phoci = 0.65 atm ? (10 points) Cl20 (g) + H2O (g) = 2 HOCl2 (g) Kp=0.085 at 395 °C 1b. Does the total pressure in the cylinder increase, decrease or remain the same as the reactions goes...

  • 1. At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant,...

    1. At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Kc, which is a mathematical expression based on the chemical equation. For example, in the reaction aA+bB⇌cC+dD where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is Kc=[C]c[D]d[A]a[B]b where [A], [B], [C], and [D] are the equilibrium concentrations. If the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, Qc, instead...

  • The initial concentrations or pressures of reactants and products are given for each of the following...

    The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. 2NH3(g)⇌N2(g)+3H2(g)Kc=17; [NH3] = 0.20 M, [N2] = 1.00 M, [H2] = 1.00 M (b) 2NH3(g)⇌N2(g)+3H2(g)KP=6.8×104; NH3 = 3.0 atm, N2 = 2.0 atm, H2 = 1.0 atm (c) 2SO3(g)⇌2SO2(g)+O2(g)Kc=0.230; [SO3] = 0.00 M, [SO2] = 1.00 M, [O2] = 1.00 M (d) 2SO3(g)⇌2SO2(g)+O2(g)KP=16.5; SO3 = 1.00...

  • 6) Calculate the pressures of all species at equilibrium in a mixture of NOCl, NO, and...

    6) Calculate the pressures of all species at equilibrium in a mixture of NOCl, NO, and Cl2 produced when a sample of NOCl with an initial pressure of 10.0 atm comes to equilibrium according to this reaction: 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) KP=4.0×10−4

  • Calculate the equilibrium pressures of all species in an equilibrium mixture that results from the decomposition...

    Calculate the equilibrium pressures of all species in an equilibrium mixture that results from the decomposition of H2S with an initial pressure of 0.824 atm. Use the 5% rule to prove that the change (x) is small enough to be neglected. Kp = 2.2 x 10-6 2H2S (g) ⇋ 2H2 (g) + S2 (g)

  • For a chemical system that is in dynamic equilibrium with Kc = 0.50, which of the...

    For a chemical system that is in dynamic equilibrium with Kc = 0.50, which of the following statements is FALSE? Both reactants and products are present in the reaction mixture From the perspective of the forward reaction, the reaction mixture at equilibrium lies in favor of the products The composition of the reaction mixture does not change with time The rate of conversion of reactants to products is the same as the rate of conversion of products to reactants The...

  • 3. The reaction that defines the heat of formation of carbon tetrachloride in the gas phase...

    3. The reaction that defines the heat of formation of carbon tetrachloride in the gas phase is given below and as an equilibrium has a Kp value of 1.48 at 277 °C. C (s, graphite) + 2 Cl2 (g) - CCl4 () Kp = 1.48 at 277 °C 3a. For the following initial pressures would you expect a reaction in the forward direction (towards products), reverse direction (towards reactants) or that there will be no net reaction: Pcı2 = 0.15...

  • The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the...

    The equilibrium constant, Kc, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp=Kc(RT)?n where R=0.08206 L?atm/(K?mol), T is the absolute temperature, and ?n is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction N2(g)+3H2(g)?2NH3(g) for which ?n=2?(1+3)=?2. Part A For the reaction 3A(g)+3B(g)?C(g) Kc...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT