A student ran the following reaction in the laboratory at
1185 K:
2SO2(g) +
O2(g)
2SO3(g)
When she introduced 8.07×10-2 moles of
SO2(g) and
7.94×10-2 moles of
O2(g) into a 1.00 liter container, she
found the equilibrium concentration of
O2(g) to be
5.86×10-2 M.
Calculate the equilibrium constant, Kc, she obtained for
this reaction.
Kc=?
A student ran the following reaction in the laboratory at 1185 K: 2SO2(g) + O2(g) 2SO3(g)...
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...
A student ran the following reaction in the laboratory at 293 K: 2CH2Cl2(g) CH4(g) + CCl4(g) When she introduced 6.91×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.19×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
A student ran the following reaction in the laboratory at 283 K: 2CH2Cl2(g) ->CH4(g) + CCl4(g) When she introduced 7.70×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.59×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
A student ran the following reaction in the laboratory at 425 K: PCl5(g) --> PCl3(g) + Cl2(g) When she introduced 4.59 moles of PCl5(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 3.94×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student ran the following reaction in the laboratory at 294 K: 2CH2Cl2(g) ____> CH4(g) + CCl4(g) When she introduced 7.04×10-2 moles of CH2Cl2(g) into a 1.00 Liter container, she found the equilibrium concentration of CCl4(g) to be 3.25×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student ran the following reaction in the laboratory at 380 K: CH4(g) + CCl4(g) 2CH2Cl2(g) When she introduced 4.26×10-2 moles of CH4(g) and 5.94×10-2 moles of CCl4(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 5.11×10-2 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 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 647 K: 2HI(g) H2(g) + I2(g) When she introduced 0.395 moles of HI(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 3.95×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.
A student ran the following reaction in the laboratory at 673 K: H2(g) + I2(g) 2HI(g) When she introduced 0.228 moles of H2(g) and 0.256 moles of I2(g) into a 1.00 liter container, she found the equilibrium concentration of I2(g) to be 6.53×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.