Chemistry

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1. Chemistry

   At T = 25 degrees Celsius, the reaction No2 2NO +O2 has an equilibrium constant K=5.0*10^-13. Suppose the container is filled with NO2 at an initial pressure of 0.25 atm. Calculate the partial pressure of NO at equilibrium

2. chemistry

   A researcher put 10.0 moles of N2O into a 2-L container at some temperature where it decomposes according to the following: N2O = 2N2+ O2. At equilibrium 2.20 moles of N2O remain. Calculate the Kc for the reaction. How am I

3. 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

4. chemistry

   Given the equilibrium constant values: N2 + 1/2O2 >>> N2O ; kc = 2.7 * 10^-18 N2O4>>>>2NO2 kc=4.6*10^-3 1/2N2 + O2>>>NO2 kc = 4.1 * 10^-9 What is a value of Kc for this reaction? 2N2O + 3O2 >>> 2N2O4

1. Chemistry

   Which of the following statements is true regarding the dissolution of a salt in a solvent? A. Precipitates are included in the equilibrium constant. B. An equilibrium constant can be describes that is the product of the

2. Chemistry

   The equilibrium constant for the reaction H2 + I2 --> 2HI, is 54 at 425 degrees C. If the equilibrium mixture contains 0.030 M HI and 0.015 M I2, calculate the equilibrium concentration of H2.

3. chem

   a.) At equilibrium, the molar concentrations for reactants and products are found to be [I2] = 0.50 M,[Cl2] = 0.60 M, and [ICl] = 5.0 M. What is the equilibrium constant (Kc) for this reaction? b.) The concentration of I2 is

4. chemistry

   Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g), increasing the concentration of the Fe(s) would: Answer A. Shift the equilibrium to the right B. Shift the equilibrium to the left C. No change

1. Chemistry

   At 55C, the K for the reaction: 2NO2(g) N2O4 is 1.15 a) write the equilibrium expression b) calculate the concentration of N2O4(g) present in equilibrium with 0.50 mole of NO2 Please help and explain

2. chemical equilibrium

   At a certain temperature, Kc = 0.914 for the reaction NO2 (g) + NO (g) N2O (g) + O2 (g) Equal amounts of NO and NO2 are to be placed in a 5.00 L container until the N2O concentration at equilibrium is 0.050 M. How many moles of NO

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. chem help!

   The equilibrium constant, Kc, for the equilibrium N2O4(g)←→2NO2(g) is 4.6×10−3 . If the equilibrium mixture contains 5.0×10−2M NO2, what is the concentration of N2O4?

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