When she introduced 0.142 moles of NO(g) and 0.112 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.107 M.
When she introduced 0.142 moles of NO(g) and 0.112 moles of Br2(g) into a 1.00 liter...
A student ran the following reaction in the laboratory at 254 K: 2NO(g) + Br2(g) ⇌ 2NOBr(g) When she introduced 0.185 moles of NO(g) and 0.130 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.152 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
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...
A student ran the following reaction in the laboratory at 225 K: 2NOBr(g) 2 2NO(g) + Brz(g) When she introduced 0.198 moles of NOBr(g) into a 1.00 liter container, she found the equilibrium concentration of Br2(g) to be 1.89x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
A student ran the following reaction in the laboratory at 324 K: 2NO(g) + Br2(g) 2NOBr(g) When she introduced 0.137 moles of NO(g) and 0.119 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of Br2(g) to be 6.92×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student ran the following reaction in the laboratory at 325 K 2NO(8) + Br2(e)2NOBr(g) When she introduced 0.120 moles of NO(g) and 9.52x102 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of Br2(g) to be 5.35x102 M. Calculate the equilibrium constant, Kg, she obtained for this reaction. Ke
A student ran the following reaction in the laboratory at 686 K: H2(g) + I2(g) 2HI(g) When she introduced 0.200 moles of H2(g) and 0.230 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.18×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
A student ran the following reaction in the laboratory at 330 K: 2NO(g) + Br (9) 2 2NOBr(g) When she introduced 0.103 moles of NO(g) and 9.25x10-- moles of Br (9) into a 1.00 liter container, she found the equilibrium concentration of Br2(g) to be 5.67x10-2 M. Calculate the equilibrium constant. Ko she obtained for this reaction. K =|
The box in the reaction equation is an equilibrium sign. ulat... 2req A student ran the following reaction in the laboratory at 726 K: ration ion ion N2(g)+3H2(g) 2NH3(g) ion When she introduced 3.30x 10-2 moles of N2(g) and 6.61x102 moles of H2(g) into a 1.00 liter container, pulati... M) M) ng Eq... she found the equilibrium concentration of H2(g) to be 6.44x102 M ibri... 2req Calculate the equilibrium constant, Kç, she obtained ng Eq... for this reaction tio... 2req...
Use the References to access impertant values if needed for A student ran the following reaction in the laboratory at 232 K: 2NOBr(g) 2NO(g)+ Br(g) When she introduced 0.138 moles of NOBr(g) into a 1.00 liter container, she found the equillibrium concentration of Bry(g) to be 1.56x102 M. Calculate the equilibrium constant, Ke, she obtained for this reaction. Kg Submit Answer 4 question attempts remaining
1. A student ran the following reaction in the laboratory at 632 K: 2HI(g) ->H2(g) + I2(g) When she introduced 0.362 moles of HI(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 3.55×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = 2. A student ran the following reaction in the laboratory at 616 K: CO(g) + Cl2(g) -> COCl2(g) When she introduced 0.131 moles of CO(g) and 0.161 moles...