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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 72

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)

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

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

Multiple Choice

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

Correct Answer:
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Unlock this answer now
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