H2(g) + Cl2(g) 2 HCl(g) Which item is being reduced in this reaction? thanks
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H2(g) + Cl2(g) 2 HCl(g) Which item is being reduced in this reaction? thanks
For the reaction H2(g) +
Cl2(g) 2 HCl(g), the
equilibrium constant K at 800oC is 4.35 x
104.
Hydrogen and chlorine, each at a partial pressure of 0.700 bar,
are placed in a vessel at 800oC and allowed to
equilibrate. Find the final partial pressures of all three gases in
this reaction.
p(H2) = bar
p(Cl2) =
. bar
p(HCl) =
bar
In the Given the redox reaction: 2Cs(s) + Cl2(g) 2C8C1(5). Cl2 is: a. Being reduced by gaining electrons b. Being oxidizing by losing electrons c. Being reduced by losing electrons d. Being oxidizing by gaining electrons e. None of these
For the reaction H2(g) + Cl2(g) 2 HCl(g), the equilibrium constant K at 800oC is 4.35 x 10^4. Hydrogen at a partial pressure of 0.700 bar and chlorine at a partial pressure of 0.500 bar are placed in a vessel at 800oC and allowed to equilibrate. Find the final partial pressures of all three gases in this reaction in bar
A student measures the reaction H2(g) + Cl2(g) <=> 2 HCl(g) concentrations at a few different temperatures and obtains the equilibrium constant. The student wants to use the van't Hoff equation to roughly determine the reaction enthalpy assuming that it does not change over the region of interest. T(K) 300 500 1000 Keq 4x1031 4x108 So the student plots the data in the Ink vs 1/T diagram and obtains a linear fitting shown below: 80 4x1018 60 In(K) 40 20...
H2(g) + Cl2(g) ↔ 2 HCl(g) If the initial concentration of HCl is 0.263 M and the equilibrium constant Kc = 0.381, what is the Cl2 concentration at equilibrium? Answer to 3 decimal places
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