An ideal gas occupies $6.00 \times 10 ^ { 2 } \mathrm {~cm} ^ { 3 } \text { at } 20 ^ { \circ } \mathrm { C }$ At what temperature will it occupy $1.20 \times 10 ^ { 3 } \mathrm {~cm} ^ { 3 }$ if the pressure is held constant?
A) $100 ^ { \circ } \mathrm { C }$
B) $313 ^ { \circ } \mathrm { C }$
C) $10 ^ { \circ } \mathrm { C }$
D) $40 ^ { \circ } \mathrm { C }$

Question

Quizplus · Accepted Answer

Charles's law states that the volume of an ideal gas is directly proportional to its absolute temperature, provided that the pressure remains constant. Mathematically, this can be expressed as:V/T = constantwhere V is the volume of the gas and T is its absolute temperature.In this problem, we are given that the volume of the gas increases from 600 cm^3 to 1200 cm^3, while the pressure remains constant. This means that the ratio V/T must remain constant.Therefore, we can write:V1/T1 = V2/T2where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.Substituting the given values, we get:600 cm^3 / (20 + 273) K = 1200 cm^3 / T2Solving for T2, we get:T2 = 313 KConverting to degrees Celsius, we get:T2 = 313 K - 273 K = 40 °CTherefore, the correct answer is B) 313 °C.

An Ideal Gas Occupies 6.00×102 cm3 at 20∘C6.00 \times 10 ^ { 2 } \mathrm {~cm} ^ { 3 } \text { at } 20 ^ { \circ } \mathrm { C }6.00×102 cm3 at 20∘C

An Ideal Gas Occupies $6.00 \times 10 ^ { 2 } \mathrm {~cm} ^ { 3 } \text { at } 20 ^ { \circ } \mathrm { C }$