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The Volume of a gas is measured to be 675.6 mL at 61.8 C. If the volume of the gas were changed to 410.9 mL, what would the final temperature be?

User Harkish
by
7.7k points

1 Answer

4 votes

Answer:

203.63 K

Step-by-step explanation:

Using Charles law equation,

V1/T1 = V2/T2

Where;

V1 = initial volume (mL)

V2 = final volume (mL)

T1 = initial temperature (K)

T2 = final temperature (K)

According to the information in this question,

V1 = 675.6 mL

V2 = 410.9 mL

T1 = 61.8°C = 61.8 + 273 = 334.8K

T2 = ?

Using V1/T1 = V2/T2

675.6/334.8 = 410.9/T2

Cross multiply

675.6 × T2 = 334.8 × 410.9

675.6T2 = 137569.32

T2 = 137569.32 ÷ 675.6

T2 = 203.63 K

User Walt Howard
by
8.2k points
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