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NOCL(g) decomposes to from nitrogen
Nitrosyl chloride (NOCl)decomposes to nitrogen oxide and chlorine gases.
The concentration of NOCl drops from 0.580 M to 0.238 M
2 answers
asked by
Caden
1,353 views
NOCL(g) decomposes to from nitrogen monoxide gas and chlorine gas. The equation is
2NOCL ----> 2NO +Cl2 At a certain temperature
2 answers
asked by
Maeve
1,327 views
The compound NOCl decomposes to nitric oxide and chlorine according to the following equation:
2 NOCl (g) → 2 NO (g) + Cl2 (g)
7 answers
asked by
John
1,238 views
Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is
2 NOCl (g) -> 2 NO (g) + Cl2 (g) at 227C Using delta H =
5 answers
asked by
CHRIS
1,221 views
Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is
2 NOCl (g) -> 2 NO (g) + Cl2 (g) at 227C Using delta H =
0 answers
asked by
CHRIS
562 views
1) Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is
2 NOCl (g) -> 2 NO (g) + Cl2 (g) at 227oC Using delta
2 answers
asked by
Hannah
977 views
1) Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is
2 NOCl (g) -> 2 NO (g) + Cl2 (g) at 227oC Using delta
3 answers
asked by
Hannah
675 views
I have been at this question for at least three hours now.
Consider the chemical system below. 2 NOCl(g) 2 NO(g) + Cl2(g) K = 1.6
3 answers
asked by
Im so sick of this problem
644 views
0.500 moles of NOCl is placed in a 1.00L vessel at 700K,and after the system comes to equilibrium,the concentration of the NOCl
0 answers
asked by
Bob
609 views
At 35°C, K = 1.6 10-5 mol/L for the following reaction.
2 NOCl(g) 2 NO(g) + Cl2(g) Calculate the concentrations of all species
0 answers
asked by
BETH
710 views