The equilibrium constant, Kc, for the following reaction is 2.0. If the equilibrium mixture contains 1.5 M NO and 1.5 M Br2, what is the molar concentration of NOBr?
2NOBr(g)⇌2NO(g)+Br2(g)
Express your answer in two significant figures
The equilibrium constant, Kc, for the following reaction is 2.0. If the equilibrium mixture contains 1.5...
The equilibrium constant, Kc, for the following reaction is 2.0. If the equilibrium mixture contains 2.3 M NO and 0.80 M Br2 , what is the molar concentration of NOBr? 2NOBr(g) = 2NO(g) + Br2 (g) Express your answer to two significant figures and include the appropriate units. Å R 0 2 ? [NOBr] = Value Units Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
For the following reaction, the equilibrium constant Kc is 0.60 at a certain temperature. If the concentration of NO(g) and NOBr(g) are both 0.10 M, at equilibrium, what is the concentration of Br2(g)? 2NO(g) + Br2(g) ⇌ 2NOBr(g)
The equilibrium constant, Kc, for the following reaction is 1.28×10-3 at 231 K. 2NOBr(g) goes to 2NO(g) + Br2(g) . When a sufficiently large sample of NOBr(g) is introduced into an evacuated vessel at 231 K, the equilibrium concentration of Br2(g) is found to be 0.200 M. Calculate the concentration of NOBr in the equilibrium mixture. __M
The equilibrium constant, Kc, for the following reaction is 6.50×10-3 at 298K. 2NOBr(g) 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 11.1 L container at 298K contains 0.376 mol of NOBr(g) and 0.396 mol of NO, the equilibrium concentration of Br2
1.The equilibrium constant, Kc, for the reaction of iodine bromide to form iodine and bromine is 2.5*10^-3. If an equilibrium mixture contains 0.58 M IBr and 3.8*10^-2 M I2, what is the molar concentration of Br2? 2IBr(g)—>I2(g)+Br2(g) express answer to two significant figures and include the appropriate units. 2. For the reaction at 225 degrees celsius at the equilibrium contant at 1.7*10^2. If the equilibrium mixture contains 0.24 M H2 and 0.025 M N2, what is the molar concentration of...
The equilibrium constant, Kc, for the reaction N2O4(g)⇌2NO2(g) is 5.1×10−3. If the equilibrium mixture contains [NO2] = 0.047 M , what is the molar concentration of N2O4? Express the concentration to two significant figures and include the appropriate units.
(a) Write the expression for the equilibrium constant (Kc) (b) Find Kc, when the equilibrium concentrations for NOBr, NO and Br2 are 0.46 M, 0.1 M and 0.3 M respectively. Report to 3 Significant figures. (c) Find Kp for the abovementioned reaction at 25°C. (R=0.082 L. atm/mole.K) (d) Find Kc, for this reaction: NO(g) + 1/2 Br2 (g) <-> NOBr (g) 1. Consider this reaction to answer the following questions touteiluna ada se in contain yo. 2NOBr (g) 2NO(g) +...
Consider the following reaction: 2NO(g)+Br2(g)⇌2NOBr(g) ,Kp=28.4, at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 102 torr and that of Br2 is 134 torr . Part A What is the partial pressure of NOBr in this mixture? Express your answer in torrs to three significant figures.
The equilibrium constant, Kc, for the following reaction is 6.50X10-3 at 298K. 2NOBr(g) =2NO(g) + Bra(g) If an equilibrium mixture of the three gases in a 11.0 L container at 298K contains 0.270 mol of NOBr(g) and 0.214 mol of NO, the equilibrium concentration of Bra is M. Submit Answer Retry Entire Group 6 more group attempts remaining
A student ran the following reaction in the laboratory at 295 K: 2NO(g) + Br2(g) <---> 2NOBr(g) When she introduced 0.153 moles of NO(g) and 0.123 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.117 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = ____ The equilibrium constant, Kc, for the following reaction is 6.50×10-3 at 298K. 2NOBr(g) <---> 2NO(g) + Br2(g) If an equilibrium mixture of...