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2 years ago

Which statement best compares the energy involved in melting with the energy involved in boiling for a given liquid?

Chemistry

2 answers:

Soloha48 [4]2 years ago

4 0

C its c trust me i just took the quiz

ruslelena [56]2 years ago

3 0

Answer is: Energy is added to the particles in each change, but boiling requires more energy than melting because the attractions must be completely overcome.

For example, melting point of the water is 0°C and boiling point of the water is 100°C.

While melting, solid water (ice) is changed into liquid water.

While boiling, liquid water is changed into gaseous water (water steam).

Between molecules of water there are hydrogen bonds, which must be brake so water can evaporate.

Hydrogen bond is an electrostatic attraction between two polar groups in which one group has hydrogen atom (H) and another group has highly electronegative atom such as nitrogen (like in this molecule), oxygen (O) or fluorine (F).

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Using the information in the table to the right, calculate the enthalpy of combustion of each of the following substances:

elena55 [62]

Answer:

Acetylene: -1,256 kJ/mol

Ethanol: -1,277 kJ/mol

The combustion of 0.25 mol of an unknown organic compound results in the release of 320 kJ of energy. Which of the compounds in the table could be the unknown compound?- Answer: Ethanol

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2 years ago

How many grams of NO are required to produce 145 g of N2 in the following reaction?

V125BC [204]

Answer:

b. 186 g

Explanation:

Step 1: Write the balanced equation.

4 NH₃(g) + 6 NO(g) → 5 N₂(g) + 6 H₂O(l)

Step 2: Calculate the moles corresponding to 145 g of N₂

The molar mass of nitrogen is 28.01 g/mol.

$145g \times \frac{1mol}{28.01 g} =5.18 mol$

Step 3: Calculate the moles of NO required to produce 5.18 moles of N₂

The molar ratio of NO to N₂ is 6:5.

$5.18molN_2 \times \frac{6molNO}{5molN_2} = 6.22molNO$

Step 4: Calculate the mass corresponding to 6.22 moles of NO

The molar mass of NO is 30.01 g/mol.

$6.22mol \times \frac{30.01g}{mol} =186 g$

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1 year ago

A mixture of gases containing 0.20 mol of SO2 and 0.20 mol of O2 in a 4.0 L flask reacts to form SO3. If the temperature is 25ºC

diamong [38]

Answer : The pressure in the flask after reaction complete is, 2.4 atm

Explanation :

To calculate the pressure in the flask after reaction is complete we are using ideal gas equation.

$PV=n_TRT\\\\P=(n_1+n_2)\times \frac{RT}{V}$

where,

P = final pressure in the flask = ?

R = gas constant = 0.0821 L.atm/mol.K

T = temperature = $25^oC=273+25=298K$

V = volume = 4.0 L

$n_1$ = moles of $SO_2$ = 0.20 mol

$n_2$ = moles of $O_2$ = 0.20 mol

Now put all the given values in the above expression, we get:

$P=(0.20+0.20)mol\times \frac{(0.0821L.atm/mol.K)\times (298K)}{4.0L}$

$P=2.4atm$

Thus, the pressure in the flask after reaction complete is, 2.4 atm

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1 year ago

What volume of 0.210 M sulfuric acid is required to completely react with 2.14 g aluminium hydroxide?

Galina-37 [17]

3 H2SO4 + 2 Al(OH)3 → Al2(SO4)3 + 6 H2O

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