Chemistry

Given the following equation:

SO2 + NO2 <--> SO3 + NO

At 25 Celcius, 2.00 mol of each of SO2 and NO2 are introduced into a 1.0L sealed flask. When euilibrium is reached, it is found that
[NO2] = 1.30 mol/L
[SO3] = 1.30 mol/L

--
Calculate the concentration at equilibrium of SO2 and NO2.



detailed answer, please, and thank you.

and Calculate the K value at 25 degrees Celcius

If 1.3 moles of each reactant is used, then 2 minus that is how much remains.

concentration = amount left/volume

asked by Lily

Respond to this Question

First Name

Your Answer

Similar Questions

  1. General Chemistry

    At a certain temperature, the equilibrium constant for the following chemical equation is 2.90. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.53 mol of SO2(g) in order to form 1.10 mol of
  2. Chemistry

    SO2(g) + NO2(g) SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. (a) What is the new equilibrium concentration of NO when 1.50
  3. Chemistry

    At a certain temperature, the equilibrium constant for the following chemical equation is 2.00. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.64 mol of SO2(g) in order to form 1.10 mol of
  4. Chemistry

    At a given temperature, analysis of an equilibrium mixture represent below is given as: SO2(g) + NO2(g) <--> SO3(g) + NO(g) Where [SO2]=4.0M, [NO2]=0.50M, [SO3]= 3.0M, [NO]=2.0M. Find the value of Keq
  5. Chemistry

    The equilibrium constant is 16 for the gas phase reaction SO2 + NO2 <--> SO3 + NO at a certain temperature. If 3.0 moles each of SO2 and NO2 are placed together in an empty 1.0 liter flask and the system is allowed to come
  6. Chemistry

    SO2(g) + NO2(g) reverse reaction arrow SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. ---How many moles/liter of NO2 would have
  7. Chem Equilbirum

    SO2(g) + NO2(g) reverse reaction arrow SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. ---How many moles/liter of NO2 would have
  8. Chemistry

    Why is sulfur dioxide (SO2) a better reducing agent than carbon dioxide (CO2) or nitrogen dioxide (NO2)? I really don't know how to answer your question. It's much like asking why the sky is blue, etc. You can look up the
  9. Chemistry

    At a particular temperature, K=3.75 for the following reaction. SO2(g) + NO2(g) (reversible arrows) SO3(g) + NO(g) If all four gases had initial concentrations of 0.500 M, calculate the equilibrium concentrations of the gases.
  10. Chemistry

    Given a sample of gas (2.49 g) with a volume of 752 mL at 335K and 1.98 atm, what is the gas, SO2 or NO2? PV=nRT (1.98atm)(0.752L)= X (0.08206L-atm/mol-K)(335K) X = 0.0541634989 mol= g/gfm 2.49/X= 0.0541634989 X = 45.97 NO2 has

More Similar Questions