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3 years ago

A liquid boils when its vapor pressure equals the pressure of the atmosphere.

Chemistry

2 answers:

max2010maxim [7]3 years ago

4 0

Answer:

True

Explanation:

The boiling point of a liquid is the temperature at which the vapour pressure of the liquid equals the pressure of the surrounding atmosphere.

When a liquid is heated, the vapour pressure gradually increases till it matches the ambient pressure. Gas bubbles begin to form within the liquid, rise to the surface and then burst up to release gas. At this point, we say the liquid is boiling.

The lower the surrounding pressure, the lower the boiling point of a liquid and vice versa. Water boils at lower temperature in high altitudes because of lower pressure as compared to sea level.

Correct option: True.

JulijaS [17]3 years ago

3 0

The answer is true. A liquid boils when its vapor pressure equals the pressure of the atmosphere. At this point, vapor can now readily escape from the liquid phase because it has an equal pressure now with its surrounding which, basically, is in the vapor phase.

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Answer:

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Explanation:

Step 1: Data given

Mass of octane = 1.00 grams

Heat capacity of calorimeter = 837 J/°C

Mass of water = 1200 grams

Temperature of water = 25.0°C

Final temperature : 33.2 °C

Step 2: Calculate heat absorbed by the calorimeter

q = c*ΔT

⇒ with c = the heat capacity of the calorimeter = 837 J/°C

⇒ with ΔT = The change of temperature = T2 - T1 = 33.2 - 25.0 : 8.2 °C

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Step 3: Calculate heat absorbed by the water

q = m*c*ΔT

⇒ m = the mass of the water = 1200 grams

⇒ c = the specific heat of water = 4.184 J/g°C

⇒ ΔT = The change in temperature = T2 - T1 = 33.2 - 25 = 8.2 °C

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Step 4: Calculate the total heat

qcalorimeter + qwater = 6863.4 + 41170. 56 = 48033.96 J = 48 kJ

Since this is an exothermic reaction, there is heat released. q is positive but ΔH is negative.

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Step 6: Calculate heat combustion for 1.00 mol of octane

ΔH = -48 kJ / 0.00875 moles

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