At 500°C the equilibrium constant,K p ,is 4.00 $\times$ 10 -4 for the equilibrium: 2HCN(g) H 2 (g)+ C 2 N 2 (g) What is K p for the following reaction? H 2 (g)+ C 2 N 2 (g) 2HCN(g)

The Answer of At 500°C the equilibrium constant,K p ,is 4.00 $\times$ 10 -4 for the equilibrium: 2HCN(g) H 2 (g)+ C 2 N 2 (g) What is K p for the following reaction? H 2 (g)+ C 2 N 2 (g) 2HCN(g)

At 500°C the equilibrium constant,K p ,is 4.00 $\times$ 10 -4 for the equilibrium: 2HCN(g) H 2 (g)+ C 2 N 2 (g) What is K p for the following reaction? H 2 (g)+ C 2 N 2 (g) 2HCN(g)

The Answer of At 500°C the equilibrium constant,K p ,is 4.00 $\times$ 10 -4 for the equilibrium: 2HCN(g) H 2 (g)+ C 2 N 2 (g) What is K p for the following reaction? H 2 (g)+ C 2 N 2 (g) 2HCN(g)

Solved

At 500°C the Equilibrium Constant,K_p,is 4 $\times$ 10^-4 for the Equilibrium:
2HCN(g)
H₂(g)+ C₂N₂(g)
What Is

Question 32

Multiple Choice

At 500°C the equilibrium constant,K_p,is 4.00 $\times$ 10^-4 for the equilibrium:
2HCN(g) $At 500°C the equilibrium constant,Kp,is 4.00 \times 10-4 for the equilibrium: 2HCN(g) H2(g) + C2N2(g) What is Kp for the following reaction? H2(g) + C2N2(g) 2HCN(g) A) 2.00 \times 10-4 B) -4.00 \times 10-4 C) 1.25 \times 103 D) 2.50 \times 103 E) 4.00 \times 104$
H₂(g) + C₂N₂(g)
What is K_p for the following reaction?
H₂(g) + C₂N₂(g) $At 500°C the equilibrium constant,Kp,is 4.00 \times 10-4 for the equilibrium: 2HCN(g) H2(g) + C2N2(g) What is Kp for the following reaction? H2(g) + C2N2(g) 2HCN(g) A) 2.00 \times 10-4 B) -4.00 \times 10-4 C) 1.25 \times 103 D) 2.50 \times 103 E) 4.00 \times 104$
2HCN(g)