Question

To three significant figures, the answer is 97800

#### Earn Coins

Coins can be redeemed for fabulous gifts.

Similar Homework Help Questions
• ### The equilibrium constant for the chemical equation N2(g) 3 H2(g)2NH3 (g) is Kp = 0.0146 at...

The equilibrium constant for the chemical equation N2(g) 3 H2(g)2NH3 (g) is Kp = 0.0146 at 183 oC. Calculate the value of Kc for the reaction at 183 °C.

• ### The equilibrium constant (Kp) for the chemical equation N2(g)+3H2(g)−⇀↽−2NH3(g) is 0.0200 bar−2 at 273 °C. Calculate...

The equilibrium constant (Kp) for the chemical equation N2(g)+3H2(g)−⇀↽−2NH3(g) is 0.0200 bar−2 at 273 °C. Calculate the value of the Kc for the reaction at 273 °C.

• ### The equilibrium constant for the chemical equation N2(g)+3H2(g)−⇀↽−2NH3(g) is Kp=0.111 at 231 ∘C. Calculate the value...

The equilibrium constant for the chemical equation N2(g)+3H2(g)−⇀↽−2NH3(g) is Kp=0.111 at 231 ∘C. Calculate the value of Kc for the reaction at 231 ∘C.

• ### The equilibrium constant for the chemical equation N,(g) + 3H2(8) - 2NH3(g) is Kp = 0.0881...

The equilibrium constant for the chemical equation N,(g) + 3H2(8) - 2NH3(g) is Kp = 0.0881 at 225 °C. Calculate the value of K, for the reaction at 225°C. Kc =

• ### Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give...

Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give the following information (298.15 K) NO (g) +1/2Br2(g) NOBr(g) Ke 4.5 2 NO (g)N2(g) 02(g) Ke 3.0 x 102 5. For the BrCl decomposition reaction 2BrCl(g) Br2(g Cl2(g) Initially, the vessel is charged at 500 K with BrCl at a partial pressure of 0.500 atm. At equilibrium, the partial pressure of BrC is 0.040 atm. Calculate Kp value at 500K Consider the...

• ### The equilibrium constant for the chemical equation N2(g)+3H2(g)↽−−⇀2NH3(g) is ?p=0.0752 at 221 ∘C. Calculate the value...

The equilibrium constant for the chemical equation N2(g)+3H2(g)↽−−⇀2NH3(g) is ?p=0.0752 at 221 ∘C. Calculate the value of ?c for the reaction at 221 ∘C.

• ### 2. At 55°C, the equilibrium constant for the reaction N2(g) + 3H2(g) + 2NH3(g) is Kp=0.05....

2. At 55°C, the equilibrium constant for the reaction N2(g) + 3H2(g) + 2NH3(g) is Kp=0.05. What is the equilibrium constants Kc and Kp for the reaction 4NH3 + 2N2(g) + 6H2(g)? Kp = 400 Kc = 7.62 x 10 3. For the reaction given below, 10.00 moles of A and 25.00 moles of B are placed in a 5.00-L container at 120 °C. A(g) +2B(g) → C(g) At equilibrium, the concentration of A is 0.5 mol/L. What is the...

• ### 1. For the reaction: N2(g)+ 3H2g) 2NH3(g) 4H=-92.4 kJ Complete the Table below by writing: increase,...

1. For the reaction: N2(g)+ 3H2g) 2NH3(g) 4H=-92.4 kJ Complete the Table below by writing: increase, decrease, or no change (2p) к, Partial pressure of NH\$(PNH) The temperature is decreased The total volume is increased 2. N;(g)+Og) 2 NO(g) Ke = 4.17 x 104 at 2000 °C. Calculate K for the following reactions: a. N:(g)+O: (g) NOg) (Ip) b. 2 NO(g) N2(g) + O2(g) (Ip) 3. N2(g)+3H:(g)2NH(g) Kp= 2.79 x 10 Calculate Ke at 472 C. (p) at 472 °C....

• ### Question 16 1 pts Consider the following endothermic reaction at equilibrium: 2NH3(e) <--> N2(g) + 3H)...

Question 16 1 pts Consider the following endothermic reaction at equilibrium: 2NH3(e) <--> N2(g) + 3H) Le Chatelier's principle predicts that adding N2 (g) to the system at equilibrium will result in a decrease in the concentration of NH3 (8) a decrease in the concentration of H2(g) an increase in the value of the equilibrium constant a lower partial pressure of N2 removal of all of the H2(g)