H2(g) + CO2(g) + 10 kcal H2O(g) + CO(g)In another experiment involving the above reaction at 1,000°C, the equilibrium concentrations were found to be:
H2(g) = 2.0 moles per liter
H2O(g) = 4.0 moles per liter
CO2(g) = 5.0 moles per liter
CO(g) = 4.0 moles per liter
What is the equilibrium constant, Keq, for this reaction?
Answers
Answer: The equilibrium constant for the given reaction is 0.8
Explanation:
Equilibrium constant is defined as the ratio of concentration of the products raised to the power its stoichiometric coefficients to the concentration of reactants raised to power its stoichiometric coefficient. It is represented as
For the general equation:
The equilibrium constant is represented as:
For the given chemical equation:
for this equation is given by:
Concentration at equilibrium of
Putting values in above equation, we get:
Hence, the equilibrium constant for the given chemical reaction is 0.8
So now we have other answers.
H20, H2, CO2 and CO
Keq reaction for each formula is 1.6
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Answers
Answer : The value of of the reaction is, 480.29 KJ.
Explanation :
Formula used :
where,
= internal energy of the reaction = ?
= enthalpy of the reaction = 483.6 KJ/mole = 483600 J
= change in the moles of the reaction = Moles of product - Moles of reactant = 3 - 2 = 1 mole
R = gas constant = 8.314 J/mole.K
T = temperature =
Now put all the given values in the above formula, we get:
Therefore, the value of of the reaction is, 480.29 KJ.
2 H2O(g) → 2 H2(g) + O2(g)
You can see that there are 2 moles of gas in the reactants and 3 moles of gas in the products.
1 moles of ideal gas occupies the same volume as 1 mole of any other ideal gas under the same conditions of temp and pressure.
Since it is done under constant temp and pressure that means the volume change will be equal to the volume of 1 mole of gas
2 moles reacts to form 3 moles
The gas equation is
PV = nRT
P = pressure
V = volume (unknown)
n = moles (1)
R = gas constant = 8.314 J K^-1 mol^-1
- the gas constant is different for different units of temp and pressure (see wikki link) in this case temp and pressure are constant, and we want to put the result in an equation that has Joules in it, so we select 8.314 JK^-1mol^-1)
T = temp in Kelvin (kelvin = deg C + 273.15
So T = 403.15 K
Now, you can see that PV is on one side of the equation, and we are looking to put PdV in our dE equation. So we can say
dE = dH -dnRT (because PV = nRT)
Also, since the gas constant is in the unit of Joules, we need to convert dH to Joules
dH = 483.6 kJ/mol = 483600 Joules/mol
dE = 483600 J/mol - (1.0 mol x 8.314 J mol^-1K-1 x 403.15 K)
dE = 483600 J/mol - 3351.77 J
dE = 480248.23 J/mol
dE = 480.2 kJ/mol
Answers
Answers
Answers
Answer:
CO₂
Explanation:
The product of the reaction is CO₂.
In a chemical reaction, the product is the substance usually found on the right hand side of the expression.
Reaction equation is given as;
C + O₂ → CO₂
In this reaction, C and O₂ are the reactants
CO₂ is the product of the reaction.
- This reaction is called a combination reaction in which two species combines to give a product.
Answers
Urea has H₂N- group attached to Carbonyl Group (C=O), and such class of comounds conataining H₂N-C=O bond are called as Amides.
Result:
So, Phenobarbital belongs to Amides.
Answers
Li2S + 2 HNO3 --> 2 LiNO3 + H2S
Li2 S + H2 N2 O2 --> Li2 N2 O5 + H2 S
Li S + H2 N2 O5 -> Li N2 O5 + H2 S
Li2 S2 + H4 N4 O10 --> Li2 N4 O10 + H4 S2
Li^2 S^2 + H^4 N^4 O^10 --> Li^2 N^4 O^10 + H^4 S^2