The equilibrium constant value for the reaction below is Kc=5.27×10-8 at a certain temperature. 2 H₂S (g) + CH₄ (g) ⇄ 4 H₂ (g) + CS₂ (g) Kc=5.27×10-8 A container is fill with gases until the following concentrations are reached H₂S = 1.800 M, CH₄ = 1.800 M, H₂ = 0.0250 M and CS₂ = 0.0250 M. Calculate the value of the reaction quotient Qc when the concentrations above are reached. Very large or very small numbers should be entered in scientific notation using the 'E' format, like your calculator. A number like 2.34×10-7 should be entered as 2.34E-7 Qc=____ In which direction will the reaction initially proceed? Answer: ____
The equilibrium constant value for the reaction below is Kc=5.27×10-8 at a certain temperature.
2 H₂S (g) + CH₄ (g) ⇄ 4 H₂ (g) + CS₂ (g) Kc=5.27×10-8
A container is fill with gases until the following concentrations are reached H₂S = 1.800 M, CH₄ = 1.800 M, H₂ = 0.0250 M and CS₂ = 0.0250 M. Calculate the value of the reaction quotient Qc when the concentrations above are reached.
Very large or very small numbers should be entered in scientific notation using the 'E' format, like your calculator. A number like 2.34×10-7 should be entered as 2.34E-7
Qc=____
In which direction will the reaction initially proceed? Answer: ____
Given,
equilibrium reaction is:
At certain temperature,
concentration of substrates is:
H₂S = 1.800 M,
CH₄ = 1.800 M,
H₂ = 0.0250 M
and
CS₂ = 0.0250 M.
What is the value of Qc?
In which direction the reaction proceeds?
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