What is the numerical value of Kc for the following reaction if the equilibrium mixture contains 0.055 M N2O4 and 0.34 M NO2? N2O4 (g) ===== 2 NO2 (g)
This is a gas phase reaction,so we can calculate the equlibrium constant in term of pressure( Kp ).But no pressure is given here, so can't calculate Kp. If we know the temperature of the reaction then we can also calculate Kc from Kp value from the following relation......
=change of coefficient of the reactant and product.
Here we have to caculate the Kc value from the direct formula of Kc.
What is the numerical value of Kc for the following reaction if the equilibrium mixture contains...
What is the numerical value of Kc for the following reaction if the equilibrium mixture contains 0.055 M N2O4 and 0.34 M NO2? N2O4 (g) ===== 2NO2 (g)
The equilibrium constant, Kc, for the reaction N2O4(g)⇌2NO2(g) is 5.1×10−3. If the equilibrium mixture contains [NO2] = 0.047 M , what is the molar concentration of N2O4? Express the concentration to two significant figures and include the appropriate units.
Consider the following reaction: N2O4(g)⇌2NO2(g),Kc=0.36 at 2000∘C The reaction mixture initially contains only the reactant, [N2O4]=0.0300M , and no NO2. Find the equilibrium concentration of N2O4. Find the equilibrium concentration of NO2.
The value of Kc for the the following reaction is 0.470 at 471 K. N2O4(g)---->2NO2(g) Part 1) If a reaction vessel at that temperature initially contains 0.0200 M NO2 and 0.0200 M N2O4, what is the concentration of NO2 at equilibrium? _______M? part 2) What is the concentration of N2O4 at equilibrium? _______M?
The value of Kc for the the following reaction is 0.470 at 473 K. N2O4 = 2NO2 If a reaction vessel at that temperature initially contains 0.0250 M NO2 and 0.0250 M N2O4, what is the concentration of NO2 at equilibrium? What is the concentration of N2O4 at equilibrium?
The equilibrium constant, Kc, for the following reaction is 2.0. If the equilibrium mixture contains 1.5 M NO and 1.5 M Br2, what is the molar concentration of NOBr? 2NOBr(g)⇌2NO(g)+Br2(g) Express your answer in two significant figures
The equilibrium constant, Kc, for the following reaction is 2.0. If the equilibrium mixture contains 2.3 M NO and 0.80 M Br2 , what is the molar concentration of NOBr? 2NOBr(g) = 2NO(g) + Br2 (g) Express your answer to two significant figures and include the appropriate units. Å R 0 2 ? [NOBr] = Value Units Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
Consider the equilibrium constant Kc for the reaction: N2O4(g) ↔ 2NO2(g) is 0.211 at 100°C. What is the value for the equilibrium constant is the reaction is balanced as ½ N2O4(g) ↔ NO2(g) ? A. 0.106 B. 0.459 C. 0.211 D. 0.422
The Kc for the reaction at 298 K is given N2O4(g) ⇋ 2 NO2(g) Kc = 5.9 × 10–3 What is the Kc for the following reaction? ½ N2O4(g) ⇋ NO2(g) Kc = ?
Part A What is the numerical value of Ke for the following reaction of the equilibrium mixture at 750 C contains 0.23 M CO and 0.054 M CO Feo(@+ CO(9) Fe() +0,6) "Express your answer using two significant figures. AXO Submit Bequent Ant