Answer:
The answer is explained below:
Explanation:
Given the chemical equation:
N2H4(g)+H2(g)→2NH3(g)
The standard enthalpy of formation is given by the following formula:
ΔH^0 rxn = ∑ B reactants - ∑ product
-187.78 kJ/mol = [( 1x B N-N) + (1 x B N-H ) + (1 x b H-H)] - [ 6 x B N-H]
-187.78 kJ/mol = [( 1x B N-N) +(4 x 391 kJ/mol) + (1 x 436 kJ/mol)] - [ 6x 391 kJ/mol ]
-187.78 kJ/mol = B N-N + (1564 + 436 - 2346) kJ/mol
B = 158.22 kJ/mol
So, in this case the enthalpy of N-N bond is 158 kJ/mol
Answer:
Sulphur
Explanation
Rhombic and monoclinic sulphur are its allotropic forms
Le Châtelier's principle tells us that chemical <span>c. equilibrium </span>will adjust in an attempt to remove a stressor.
Answer:
See below
Explanation:
From periodic table, find Mole Weight of the element in question
this is the grams of the element in Avagadro's Number (6.022 x 10^23) of atoms
(5.50 x 10^22) / (6.022 x 10^23) x mole weight = grams
Explanation:
1) refine the specimen into fine powder 2) place the smallest amount you can see in the capillary tube 3) set the voltage to increase exponentially to 200 below the predicted temperature, then adjust so that the temperature rises to 20 per minute 4) report the temperature at which the liquid first appears and the temperature at which the last crystal disappears.
