Acalorimeter contains 20.0 ml of water at 15.0 ∘c . when 1.50 g of x (a substance with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction x(s)+h2o(l)→x(aq) and the temperature of the solution increases to 25.0 ∘c . calculate the enthalpy change, δh, for this reaction per mole of x. assume that the specific heat of the resulting solution is equal to that of water [4.18 j/(g⋅∘c)], that density of water is 1.00 g/ml, and that no heat is lost to the calorimeter itself, nor to the surroundings.

ΔH(mix'g)= 42.3Kj/mole

Explanation:

ΔH = (mcΔT)water/moles X

m = mass(g) = 20ml x 1.00g/ml = 20 g

c = 4.184 j/g⁰C

ΔT = 25°C- 15°C = 10°C

moles X = (1.5g)/(76g/mole) = 0.0197 mole X

ΔH = (20g)(4.184j/g°C)(10°C)/(0.0197 mole X) = 42,300J/mole = 42.3Kj/mole (3 sig.figs.)  

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

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