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Charles Law:

Solve the following.

Give the following.

Given:

Required:

Formula:

Solution:

1. A mountain climber inhales 274.0 ml of air at a temperature of 10.0 C. What volume (in ml) will the air occupy in the mountain climber's lungs if his body temperature is 37.0 C assuming that the pressure remains the same?​

Sagot :

Sama3lidn

Charles Law

V1/T1 = V2/T2

where in, V1 = first volume

T1 = first temperature

V2 = second volume

T2 = second temperature

Given: V1 = 274mL

T1 = 283.15K

T2 = 310.15K

Note: Dealing with Temperature from each of the Gas Law must always be in Kelvin.

°C → K

10°C + 273.15K = 283.15K

37°C + 273.15K = 310.15K

Required: V2 = ?

Formula: V2 = V1T2 / T1

Note: To get the formula, apply cross-multiplication, division and cancellation of like terms using the original formula of Charles Law.

V1/T1 = V2/T2 ← cross-multiply

V1T2 = V2T1 ← divide both sides by T1

V1T2 / T1 = V2T1 / T1 ← cancel like terms

V1T2 / T1 = V2 ← final formula for V2

Solution: V2 = V1T2 / T1

= (274mL)(310.15K) / 283.15K

= 84981.1mL•K / 283.15K

= 300.13mL

Note: "K" is cancelled out, so the unit for volume will remain which is "mL"

Reminder: Cancellation of units is applicable when the other same unit is on the denominator.

Final Answer: V2 = 300.13mL

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