Physical Chemistry

posted by .

At 25.0o C, the equilibrium 2 NOBr(g) ¡ê 2 NO(g) + Br2(g) is rapidly established. When 1.10 g of NOBr is placed in a 1.0 L vessel at 25.0o C, the equilibrium pressure is 0.355 bar. Calculate the equilibrium constant K. ( P¥è = 1 bar )


Angela.
Read your post (as it posted) and tell us what the funny symbols are. P probably means pressure but what is Y with two horizontal lines on the tail of the Y, and e with a backwards accent mark?

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Physical Chemistry

    At 25.0 degree celcius, the equilibrium 2 NOBr (gas) --> 2 NO (gas) + BR2 (gas) is rapidly established. When 1.10 g of NOBr is placed in a 1.0 L vessel at 25.0 degree celcius, the equilibrium pressure is 0.355 bar. Calculate the …
  2. chem

    Nitrosyl Bromide Decomposes according to: 2NOBr(g) <=> 2NO(g) + Br2(g) *<=> is an equilibrium arrow( 1 mole each of NO and BR2 are in the flask. At equilibrium .60mol of BR2 remained. What is the number of moles of NOBr …
  3. Chemistry

    Given the elementary reaction: 2 NOBr==>2 NO + Br2 k = 0.80 Which variables obtained for this reaction will produce a straight line?
  4. chem class

    Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)(equilibrium arrow) 2NO (g) + Br2 (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.46 …
  5. chemistry

    Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)(equilibrium arrow) 2NO (g) + Br2 (g) A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained 0.46 …
  6. ap chemisrty

    Kp for the following reaction is 0.16 at 25°C. 2 NOBr(g) 2 NO(g) + Br2(g) The enthalpy change for the reaction at standard conditions is +16.3 kJ. Predict the effect of the following changes on the position of the equilibrium; that …
  7. Chemistry

    The following reaction has Kp = 109 at 25°C. 2 NO(g) + Br2(g) 2 NOBr(g) If the equilibrium partial pressure of Br2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equilibrium.
  8. AP Chem

    The following reaction has Kp = 109 at 25°C. 2 NO(g) + Br2(g) 2 NOBr(g) If the equilibrium partial pressure of Br2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equilibrium.
  9. Chemistry

    Nitrosyl bromide, NOBr, readily dissociated according to the following equilibrium equation: 2 NOBr (g) ----> 2 NO(g) + Br2 (g) NOBr was placed in a 1.00 L flask at 25.0oC and allowed to dissociated. At equilibrium, 0.17 moles of …
  10. Chemistry 2

    Pure nitrosyl bromide, NOBr at 0.762 M is placed into a sealed vessel and heated up to 400 K. When the system reaches equilibrium, it is found that 65.1% of the nitrosyl bromide has decomposed to nitrogen monoxide and bromine. Determine …

More Similar Questions