Suppose the ΔGof, ΔHof, and ΔSo are available and valid at 298 K. Which equation(s) would...
Suppose the ΔGof, ΔHof, and ΔSo are available and valid at 298 K. Which equation(s) would be used during the calculation of the ΔG if all product concentrations are 3 M and all reactant concentrations are 2 M and the temperature is 600 K? Choose all that apply.
ΔGo= -RT ln K
ΔGo=ΔHo-TΔSo
ΔG=ΔGo+RT ln Q
ΔGo=ΣΔGof(products)-ΣΔGof(reactants)
Homework Answers
First we can calculate the ΔGo with the help of ΔGo=ΣΔGof(products)-ΣΔGof(reactants) equation.
now , for calculating the ΔG,
we can use ΔG=ΔGo+RT ln Q equation.
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Suppose the ΔGof, ΔHof, and ΔSo are available and valid at 298
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1) At 298 K, an equilibrium
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You must show all your work to receive credit. Watch sig figs! Consider the reaction: 1) At 298 K, an equilibrium mixture contains P H2-0.958 atm, P ½=0.877 atm, and P HI-0.020 atm. Calculate the value of the equilibrium constant Kp? a) (o, o2) 0.938x o.87? b) And what is the value of the equilibrium constant...
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Please show all of the steps.
The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard- state conditions, the equation is E = E – 2.303 RT logo ne where is the potential in volts, E is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q...
1) At 298 K, an equilibrium
mixture contains P H2=0.958 atm, P I2= 0.877 atm and P HI=0.020
atm. Please try and answer all!
You must show all your work to receive credit. Watch sig figs! Consider the reaction: 1) At 298 K, an equilibrium mixture contains P H2-0.958 atm, P ½=0.877 atm, and P HI-0.020 atm. Calculate the value of the equilibrium constant Kp? a) (o, o2) 0.938x o.87? b) And what is the value of the equilibrium constant...
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