and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas. moléš of oxygen (O2) gas in a 7.95 Liter air tight metal flask at 127 Now that you have calculated the K. value which way will the chemical equilibrium shift? left and then right and favor products left and then right and favor reactants at equilibrium and favor neither at equilibrium and favor reactants can't be determined right and favor products right and then left and favor reactants right and then left and favor products at equilibrium and favor products right and favor reactants left and favor products left and favor reactant O O O C
and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas. moléš of oxygen (O2) gas in a 7.95 Liter air tight metal flask at 127 Now that you have calculated the K. value which way will the chemical equilibrium shift? left and then right and favor products left and then right and favor reactants at equilibrium and favor neither at equilibrium and favor reactants can't be determined right and favor products right and then left and favor reactants right and then left and favor products at equilibrium and favor products right and favor reactants left and favor products left and favor reactant O O O C
and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas. moléš of oxygen (O2) gas in a 7.95 Liter air tight metal flask at 127 Now that you have calculated the K. value which way will the chemical equilibrium shift? left and then right and favor products left and then right and favor reactants at equilibrium and favor neither at equilibrium and favor reactants can't be determined right and favor products right and then left and favor reactants right and then left and favor products at equilibrium and favor products right and favor reactants left and favor products left and favor reactant O O O C
If a chemist mixed 2.930 moles of ammonia (NH3) gas with 1.978 moles of oxygen (O2) gas in a 7.95 Liter air tight metal flask at 127°C and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas. Now that you have calculated the Kc value use the equation Kp = Kc (RT)∆^ n to solve for Kp value
If a chemist mixed 2.930 moles of ammonia (NH3) gas with 1.978 moles of oxygen (O2) gas in a 7.95 Liter air tight metal flask at 127°C and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas. Now that you have calculated the Kc value which way will the chemical equilibrium shift?
Transcribed Image Text:as Prepared...
nitrogen n2 is soluble in bl...
Nitrogen, N2, Is Soluble In.
housto
4NH3(g) + 302(g)
= 2N2(g) + 6H2O(g)
If a chemist mixed 2.930 moles of ammonia (NH3) gas with 1.978 moles of oxygen (O2) gas in a 7.95 Liter air tight metal flask at 127°C
and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas.
Now that you have calculated the K. value which way will the chemical equilibrium shift?
Oleft and then right and favor products
O left and then right and favor reactants
at equilibrium and favor neither
at equilibrium and favor reactants
can't be determined
right and favor products
right and then left and favor reactants
right and then left and favor products
at equilibrium and favor products
O right and favor reactants
Oleft and favor products
O left and favor reactant
Transcribed Image Text:in bl...
Nitrogen, N2, Is Soluble In...
4NH3(g) + 302(g)
= 2N2(g) + 6H2O(g)
If a chemist mixed 2.930 moles of ammonia (NH3) gas with 1.978 moles of oxygen (O2) gas in a 7.95 Liter air tight metal flask at
and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas.
Now that you have calculated the Kc value use the equation Kp = Kc (RT)A^ to solve for the Kp value.
%3D
O 20.35
34.85
38.74
36.68
O 18.06
29.93
32.16
23.84
30.35
25.54
O 27.49
01639
Definition Definition State where the components involved in a reversible reaction, namely reactants and product, do not change concentration any further with time. Chemical equilibrium results when the rate of the forward reaction becomes equal to the rate of the reverse reaction.
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