# chemistry

For 2SO2(g)+O2(g)⇌2SO3(g),
Kp=3.0×104 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.15 g of SO3 and 0.107 g of O2.

1) How many grams of SO2 are in the vessel?

----------------------------

A flask is charged with 1.500 atm of N2O4(g) and 1.00 atm NO2(g) at 25 ∘C, and the following equilibrium is achieved:
N2O4(g)⇌2NO2
After equilibrium is reached, the partial pressure of NO2 is 0.519 atm .

2) Calculate Kc for the reaction.

-----------------------------

3) Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas:
PCl3(g)+Cl2(g)⇌PCl5(g).
A 7.5-L gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibrate at 450 K. At equilibrium the partial pressures of the three gases are PPCl3 = 0.128 atm , PCl2 = 0.159 atm , and PPCl5 = 1.90 atm .

Calculate Kc for this reaction at 450 K.

1. 👍
2. 👎
3. 👁
4. ℹ️
5. 🚩
1. A flask is charged with 1.500 atm of N2O4(g) and 1.00 atm NO2(g) at 25 ∘C, and the following equilibrium is achieved:
N2O4(g)⇌2NO2
After equilibrium is reached, the partial pressure of NO2 is 0.519 atm . Calculate Kc.

........N2O4 ⇌ 2NO2
I.......1.5.....1.0
C.......+p......-2p
E......1.5+p....1.0-2p

You know 1.0-2p = 0.519. Solve for p. KNowing p you calculate pN2O4 at equilibrium. Write Kp expression, substitute the equilibrium values and solve for Kp. Convert to Kc using Kp = Kc(RT)^delta n.
Post your work if you get stuck.

1. 👍
2. 👎
3. ℹ️
4. 🚩
2. It appers to me that the easy way is to solve for Kp since partial pressure of each gas is given at equilibrium, then convert to Kc.

If you want to do it the longer way, use PV = nRT and solve for n for each gas, then convert to M using M = mols/L. Then plug into the Kc expression and solve for Kc
Post your work if you get stuck.

1. 👍
2. 👎
3. ℹ️
4. 🚩
3. Here is #1,
For 2SO2(g)+O2(g)⇌2SO3(g),
Kp=3.0×104 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.15 g of SO3 and 0.107 g of O2.

Use PV - nRT and calculate pSO3.
Use PV = nRT and calculate pO2
Write the Kp expression, substitute the partial pressures of SO3 and O2 and calculate pSO2. Then use PV = nRT and solve for mols SO2 and convert to grams SO2. Post your work if you get stuck.

1. 👍
2. 👎
3. ℹ️
4. 🚩
4. I've worked this problem several times and keep getting the wrong answer. I've got .035, .0255, and 51.04. Are any of these close?

1. 👍
2. 👎
3. ℹ️
4. 🚩

## Similar Questions

1. ### chemistry

In the reaction 2SO2 (g) + O2 (g) 2SO3 (g), which change would cause the greatest increase in the concentration of SO3?

2. ### chemistry

For the following reaction, 2SO3(g) = 2SO2(g) + O2(g), the equilibrium constant, Kp, is 1.32 at 627 degrees Celsius. What is the equilibrium constant for the reaction: SO3(g) = SO2(g)+ 1/2 O2(g)

3. ### Chemistry

Calculate the enthalpy change for the reaction: 2S(s) + 3O2(g) --> 2SO3(g) Use the following thermochemical equations: Reaction S(s) + O2(g) --> SO2(g) Delta H(in kJ) -296.8 2SO2(g) + O2(g) --> 2SO3(g) Delta H(in kJ) -197.0

4. ### Chemistry

For the reaction, 2SO2(g) + O2(g) ¨ 2SO3(g) + heat, at equilibrium, what will be the effect on the net amount of SO3 present if the temperature of the container is increased? A) The concentration of SO3 decreases. B) The

1. ### Chemistry

If the reaction SO2(g) +0.5O2(g) SO3(g) has the equilibrium constant Kc =56, then what is the Kc value for the following reaction? 2SO3 (g) 2SO2 (g) + O2(g) A. -112 B. 3.2 * 10^-4 C. 56 D. 8.9*10^-3 I think the answer would be C

2. ### AP Chemistry

For the system 2SO2(g) + O2(g) 2SO3 (g), change in enthalpy is negative for the production of SO3. At a particular temperature, 8.00 moles of sulfur dioxide and 10.00 moles of sulfur trioxide are introduced into a 2.00 L

3. ### Chemistry

Sulfur dioxide reacts with oxygen to form sulfur trioxide according to the equation 2SO2(g) + O2(g) 2SO3(g) Samples of sulfur dioxide, oxygen, and sulfur trioxide were added to a flask of volume 1.40 dm^3 and allowed to reach

4. ### Chemistry

If the reaction SO2(g) + ½O2(g) SO3 (g) has the equilibrium constant Kc = 56, then what is the value of Kc for the following reaction? 2SO3(g) 2SO2(g) + O2(g) A. 3.2 × 10-4 B. -112 C. 8.9 × 10-3 D. 56

1. ### Chemistry

At 1285°C, the equilibrium constant for the reaction Br2 (gas) 2Br (gas) is Keq= 1.04 X 10^ -3 A 0.200-L vessel containing an equilibrium mixture of gases has 0.245 g. Br2 (gas) in it. What is the mass of Br (gas) in the vessel?

2. ### Chemistry

The equilibrium constant is equal to 5.00 at 1300K for the reaction 2SO2(g) + O2(g) 2SO3(g) if initial concentrations are [SO2] = 6.00M, [O2] = 0.45M, [SO3]= 9.00M, the system is a/. At equilibrium b/. Not at equilibrium and will

3. ### chem

(a) At 800 K the equilibrium constant for I2(g) 2 I(g) is Kc = 3.1 10-5. If an equilibrium mixture in a 10.0-L vessel contains 3.25 10-2 g of I(g), how many grams of I2 are in the mixture? (b) For 2 SO2(g) + O2(g) 2 SO3(g), Kp =

4. ### Chemistry

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g). 2SO2(g)+O2(g)=2SO3(g) Kc=1.7*10^8 [SO3]aq=0.0034 M [O2]aq=0.0018