Calculate the mass of methane that must be burned to provide enough heat to convert 300.0...

Calculate the mass of methane that must be burned to provide enough heat to convert 300.0 g of water at 30.0°C into steam at 106.0°C.

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Expert Solution

the enthapy of combustiondata of methane and the enthapy of vaporisation of water should be given.

these data are missing so i am taking them from my side .....

CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O (l) ΔH combustion = - 890Kj/mol

H2O(l) --------> H2O (g) ΔHvap = 40.66 kj/mol

Specific heat of water = 4.184 j/g Specific heat of steam = -1.996 j/g

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Heat needed for Water = Heating from 30^o to 100^o + heat for vaporisation at 100^o +

heat for heating steam from 100^o to 106^o

= (msΔT)_water + n x ΔHvap + (msΔT )_steam

= 300x4.184x (100-30) + 1000x (300/18) x40.66 + 300x(-1.996) (106-100)

= 24864 + 677666.67 - 3592.8 =698.937 Kj

Heat needed = heat supplied by methane

let m be the mass of the methane , so moles = m/16

698.937 Kj = (m/16) (890)

m = mass of methane = 14.921 grams

queen_honey_blossom answered 9 months ago

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