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4 years ago

What type of bond between water molecules pulls them into this tight ball?

1 answer:

6 0

A water molecule contains an oxygen atom and two hydrogen atoms which are covalently bonded to the oxygen atom.Atoms in a covalently bonded molecule are always fighting for the shared electrons, the atoms attraction to the shared electrons is called the electronegativity. Therefore, the more electronegative an atom is the more it attracts the shared electrons.The force of attraction between a partially electronegative atom and another partially positive atom is the hydrogen bond. It is the hydrogen bond that pulls water molecules together which results into a cohesive force between the water molecules.

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The fluorine-17 nuclide radioactively decays by electron capture.

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4 years ago

Which of the following is the greatest mass? Select one:

algol13

Answer:

B. 1.000 × 10-4 kg

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3 years ago

Which list contains all pure substance

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3 years ago

A spirit burner used 1.00 g methanol to raise the temperature of 100.0 g water in a metal can from 28.00C to 58.0C. Calculate th

Andreas93 [3]

Complete question:

A spirit burner used 1.00 g methanol to raise the temperature of 100.0 g water in a metal can from 28.00C to 58.0C. Calculate the heat of combustion of methanol in kJ/mol.

Answer:

the heat of combustion of the methanol is 402.31 kJ/mol

Explanation:

Given;

mass of water, $m_w$ = 100 g

initial temperature of water, t₁ = 28 ⁰C

final temperature of water, t₂ = 58 ⁰C

specific heat capacity of water = 4.184 J/g⁰C

reacting mass of the methanol, m = 1.00 g

molecular mass of methanol = 32.04 g/mol

number of moles = 1 / 32.04

= 0.0312 mol

Apply the principle of conservation of energy;

$n\Delta H_{methanol} = Q_{water}\\\\n\Delta H_{methanol} = mc\Delta t\\\\n\Delta H_{methanol} = 100 \times 4.184\times (58-28)\\\\n\Delta H_{methanol} = 12,552 \ J\\\\n\Delta H_{methanol} = 12.552 \ kJ\\\\\Delta H_{methanol} = \frac{12.552}{n} \\\\H_{methanol} = \frac{12.552 \ kJ}{0.0312 \ mol} \\\\\Delta H_{methanol} = 402.31 \ kJ/mol$

Therefore, the heat of combustion of the methanol is 402.31 kJ/mol

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3 years ago