Under constant pressure a fixed mass of a gas is heated from 0°C to 273°C. What is the ratio of the final volume of the gas with its initial volume?
Answers
Answer:
2/1 or 2:1
Explanation:
We know from the ideal gas equation that
PV = nRT
Given that P is constant and since mass is fixed, moles that is n is also constant and R is the gas constant it does not change.
Now,
PV1 = nRT1
PV2 = nRT2
PV2/PV1 = nRT2/nRT1
Therfore,
V2/V1 = T2/T1
We always keep the value of temperature in kelvin.
T2 = 273°C = 273 + 273 = 546K
T1 = 0°C = 0 + 273 = 273K
V2/V1 = T2/T1
= 546/273
=2/1 or 2:1
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using the combined gas laws. PV/T = k. Let T1 = initial temperature; T2 = the final temperature; V1 = the initial volume; V2 = the final volume; P1 = initial pressure and P2 = final pressure.
Given: T1 = 0 degrees Celsius = 273 K; P2 = 2P1; V2 = 2V1
(P1 * V1) / T1 = (P2 * V2) / T2 combined gas laws
(P1 * V1) / 273 = (2P1 * 2V1) / T2
Cancelling the common factors V1 and P1 we get
1 / 273 = 4 / T2
T2 = 273 * 4
T2 = 1092 K
T2 = 1092 – 273
T2 = 819 Celsius
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