Mass of methane takne = 1.5g
moles of methane used = masss / molar mass = 1.5 / 16 = 0.094 moles
mass of water = 1000 g
Initial temperature of water = 25 C
final temperature = 37 C
specific heat of water = 4.184 J /g C
1) Heat absorbed by water = q =m• C• ΔT = 1000 X 4.184 x (37-25) = 50208 Joules
2) Heat absorbed by calorimeter = Heat capacity X ΔT = 695 X (37-25) = 8340 J
3) Total heat of combustion = heat absorbed by water + calorimeter = 50208 + 8340 = 58548 Joules
This heat is released by 0.094 moles of methane
So heat released by one mole of methane =
- 622851.06 Joules = 622.85 kJ / mole
4) standard enthalpy of combustion = -882 kJ / mole
Error = (882-622.85) X 100 / 882 = 24.84 %
C=2
D=2
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answer
Answer:
Explanation:
Electrochemical corrosion of a metal is its spontaneous reaction with oxygen.
Let's compare the standard reduction potentials for a hypothetical metal M with that of oxygen.
<u>E°/V</u>
O₂(g) + 2H₂O(ℓ) + 4e⁻ ⇌ 4OH⁻(aq) 0.4
M²⁺(aq) + 2e⁻ ⇌ M(s) -0.1
To react spontaneously with O₂, the metal must have a
<u>E°/V
</u>
2 × [M(s) ⇌ M²⁺(aq) + 2e⁻ ] 0.1
1 × <u>[O₂(g) +2H₂O(ℓ) + 4e⁻ ⇌ 4OH⁻(aq)] </u> <u>0.4
</u>
2M(s) + O₂(g) + 2H₂O(ℓ) ⇌ 2M²⁺(aq) + 4OH⁻(aq) 0.5
Only then will we get a positive for the overall cell potential and a spontaneous reaction.
Answer:
Explanation:
Part (c)
Mix together two suitable solutions.
Use filtration to separate the precipitate as a residue from the solution.
Wash the precipitate with distilled water while it is in the filter funnel.
Leave the washed precipitate aside or in a warm oven to dry.
Part (d)
Pb(NO3)2 (aq) + Na2SO4 (aq) → 2 NaNO3 (aq) + PbSO4 (s)
Answer:
A , B, C
Explanation: D is a Diamagnetic