7:40 i 65% on.masteringchemistry.com :D The equilibrium constant, K., is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp = K.(RT)An 0.08206 L · atm/(K· mol), T is the absolute temperature, and An is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction where R N2(g) + 3H2(g) = 2NH3 (g) for which An = 2 – (1+ 3) = -2. Part A For the reaction 3A(g) + 2B(g)= C(g) Kc = 75.8 at a temperature of 75 °C. Calculate the value of Kp. Express your answer numerically. • View Available Hint(s) 7:40 session.masteringchemistry.com/myct/itemView?offset=next&attemptNo=1&ass :D

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:D
<Chapter 15 - Attempt 1
+ Pressure-Based versus Concentration-Based
Equilibrium Constants
3 of 11
<>
The equilibrium constant, K., is calculated using
molar concentrations. For gaseous reactions
another form of the equilibrium constant, Kp, is
calculated from partial pressures instead of
concentrations. These two equilibrium constants are
related by the equation
Kp = K.(RT)An
0.08206 L · atm/(K· mol), T is the
absolute temperature, and An is the change in the
number of moles of gas (sum moles products - sum
moles reactants). For example, consider the reaction
where R
N2(g) + 3H2(g) = 2NH3 (g)
for which An = 2 – (1+ 3) = -2.
Part A
For the reaction
3A(g) + 2B(g)=
C(g)
Kc = 75.8 at a temperature of 75 °C.
Calculate the value of Kp.
Express your answer numerically.
• View Available Hint(s)
Transcribed Image Text:7:40 i 65% on.masteringchemistry.com :D <Chapter 15 - Attempt 1 + Pressure-Based versus Concentration-Based Equilibrium Constants 3 of 11 <> The equilibrium constant, K., is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, Kp, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation Kp = K.(RT)An 0.08206 L · atm/(K· mol), T is the absolute temperature, and An is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction where R N2(g) + 3H2(g) = 2NH3 (g) for which An = 2 – (1+ 3) = -2. Part A For the reaction 3A(g) + 2B(g)= C(g) Kc = 75.8 at a temperature of 75 °C. Calculate the value of Kp. Express your answer numerically. • View Available Hint(s)
7:40
session.masteringchemistry.com/myct/itemView?offset=next&attemptNo=1&ass
:D
<Chapter 15 - Attempt 1
+ Pressure-Based versus Concentration-Based Equilibrium Constants
3 of 11
For the reaction
3A(g) + 2B(g) = C(g)
K. = 75.8 at a temperature of 75 °C.
Calculate the value of Kp.
Express your answer numerically.
• View Available Hint(s)
ΑΣ
Transcribed Image Text:7:40 session.masteringchemistry.com/myct/itemView?offset=next&attemptNo=1&ass :D <Chapter 15 - Attempt 1 + Pressure-Based versus Concentration-Based Equilibrium Constants 3 of 11 For the reaction 3A(g) + 2B(g) = C(g) K. = 75.8 at a temperature of 75 °C. Calculate the value of Kp. Express your answer numerically. • View Available Hint(s) ΑΣ
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