When the reaction below is at equilibrium there are 0.250 mol of Br2, 1.25 mol of Cl2, and 1.5 mol of BrCl in a closed flask of 1.00 L at 100 degrees C. A Chem 109 student upsets the equilibrium by adding 0.0500 mol of Br2 into the 1L sealed flask. The equilibrium constant for the reaction is Kc = 7.20 at 100 degrees C. Calculate the concentration of Br2, Cl2 and BrCl when the new equilibrium is established. Br2 (g) + Cl2 (g)   <--->   2 BrCl (g)                         Kc = 7.20 at 100 degrees C

Consider the following equilibrium: 2NOCl (g) <--> 2NO (g) + Cl2 (g) With K = 1.6 x 10-5. 1.00 mole of pure NOCl and 0.964 mole of pure Cl2 are placed in a 1.00 L container. Calculate the equilibrium concentration of Cl2 (g).

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 NO(g) + Cl₂(g) 2 NOC1 (g) K₂ = 1. x 10 -6 He fills a reaction vessel at this temperature with 13. atm of nitrogen monoxide gas and 17. atm of chlorine gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NOCI, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NOCI at right. Round your answer to 1 significant digit. O yes O no atm 0 X S BEEN 000 Ar

Please help.

A student ran the following reaction in the laboratory at 303 K:2NO(g) + Br2(g) 2NOBr(g)When she introduced NO(g) and Br2(g) into a 1.00 L evacuated container, so that the initial partial pressure of NO was 1.15 atm and the initial partial pressure of Br2 was 0.408 atm, she found that the equilibrium partial pressure of Br2 was 0.138 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp =

Consider the equilibrium between SbCl5, SbCl3 and Cl₂. SbCl5(g) SbCl3(g) + Cl₂(g) K = 2.46x10-² at 530 K The reaction is allowed to reach equilibrium in a 7.30-L flask. At equilibrium, [SbCl5] = 0.430 M, [SbCl3] = 0.103 M and [Cl₂] = 0.103 M. (a) The equilibrium mixture is transferred to a 14.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 14.6-L flask. [SbCl5] = [SbCl3] = [Cl₂] |||| ΣΣΣ

2. 1.00 mol of oxygen and 1.00 mol of sulfur dioxide are placed into a 1.0-L flask. Sulfur trioxide gas is formed. At 1000 K, when equilibrium has been reached, 0.93 mgl pf sulfur trioxide have been formed. What is the Kec?.

In air at 25 °C and 1.00 atm, the N₂ concentration is is 0.033 M. The 0.01 M and the O₂ concentration reaction N₂(g) + O₂(g) → 2NO(g) has Kc = 4.8 x 10-31 at 25 °C. C Taking the N₂ and O2 concentrations given above as initial values, calculate the equilibrium NO concentration that should exist in our atmosphere from this reaction at 32 °C, Kc = 2.6E-30. Make simplifying assumptions in your calculations. (Express your answer in scientific notation.) [NO] = i M !

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 6. N,(g) + 2H,0(g) 2 NO(g) + 2 H, (g) K,=7. × 10 He fills a reaction vessel at this temperature with 9.0 atm of nitrogen gas and 4.7 atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H,, using only the tools yes x10 available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of H, at right. atm Round your answer to 1 significant digit.

Can you provide an explanation? And show the steps