1.
For the reaction
2SO2(g) +
O2(g)------>2SO3(g)
H° = -198 kJ and S° = -188
J/K
The equilibrium constant, K, would be greater than 1 at
temperatures _______(above or below) ____Kelvin.
Select above or below in the first box and enter the temperature in
the second box. Assume that H° and S° are constant.
2.
How many grams of zinc metal will be deposited
from a solution that contains Zn2+ions
if a current of 0.768 A is applied for
53.1 minutes.
grams
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1. For the reaction 2SO2(g) + O2(g)------>2SO3(g) H° = -198 kJ and S° = -188 J/K...
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1260 K? Kp= ?
Consider the following equilibrium reaction. 2SO2(g)+O2(g)↽−−⇀2SO3(g)Δ?=−198 kJ/mol Which characteristics of this reaction will be affected by a change in temperature? I. value of equilibrium constant II. equilibrium concentrations Or both
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The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. 2SO3(g) 2SO2(g) + O2(g) If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1270 K? Kp =
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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=?
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