1.3 3 (ii) In the Haber process for the production of ammonia the following reaction occurs: N₂(g) 3H₂(g) 2NH3(g) DH is negative If the equilibrium concentrations for all the reactants and products at 600°C are: [N₂] = 0.40 mol/dm³, [H₂] = 1.20 mol/dm³ and [NH₂] = 0.20 mol/dm³ what is the numerical value of the equilibrium constant, K?

1.3 3 (ii) In the Haber process for the production of ammonia the following reaction occurs: N₂(g) 3H₂(g) 2NH3(g) DH is negative If the equilibrium concentrations for all the reactants and products at 600°C are: [N₂] = 0.40 mol/dm³, [H₂] = 1.20 mol/dm³ and [NH₂] = 0.20 mol/dm³ what is the numerical value of the equilibrium constant, K?

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Chapter6: Thermochemisty

Section: Chapter Questions

Problem 6.101QP: Formic acid, HCHO2, was first discovered in ants (formica is Latin for ant). In an experiment, 5.48...

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A standard dose of trinitroglycerin for relief of angina is 0.60 mg. If the sample is eventually oxidized in the body (not explosively, though!) to nitrogen gas, carbon dioxide gas, and liquid water, what number of calories is released?
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For items 1-3, refer to the equation: CH4(g) + 2O2(g) → 2H2O(l) + CO2(g), with ΔH equal to -809.94 kJ/mol.1. Is the reaction heat-producing (exothermic) or heat-absorbing(endothermic)?2. How many moles of liquid water (H2O(l)) will be produced upon combustion of 3 moles of methane gas (CH4(g))?3. Calculate the ΔH if 5g of methane gas was combusted. With solutions and explanation.
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