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To raise the temperature of one mole of a gas at constant at constant volume from 600 degree celsius to 610 degree celsius, the heat needed is 498.6 j. Which is the gas?
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To raise the temperature of one mole of a gas at constant at constant ...
Identification of Gas


To identify the gas, we need to calculate its molar specific heat at constant volume.

Calculating molar specific heat at constant volume


From the given information, we know that,

ΔT = 10°C = 10 K (change in temperature)

q = 498.6 J (heat energy)

n = 1 mol (number of moles)

Using the formula,

q = nCvΔT

We can calculate the molar specific heat at constant volume (Cv) as,

Cv = q / nΔT

Cv = (498.6 J) / (1 mol * 10 K)

Cv = 49.86 J/mol K

Comparing with Gas Constants


Now, we can compare this value of Cv with the known gas constants for different gases, such as,

- Monoatomic ideal gas: Cv = (3/2)R = 12.47 J/mol K
- Diatomic ideal gas: Cv = (5/2)R = 20.79 J/mol K
- Triatomic ideal gas: Cv = (6/2)R = 24.94 J/mol K

Since the calculated value of Cv (49.86 J/mol K) is closer to the value for a monoatomic ideal gas, we can conclude that the gas is most likely a monoatomic ideal gas.

Therefore, the gas can be Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), or Radon (Rn).

Conclusion


Based on the given information, we can conclude that the gas is most likely a monoatomic ideal gas and it can be Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), or Radon (Rn).
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To raise the temperature of one mole of a gas at constant at constant volume from 600 degree celsius to 610 degree celsius, the heat needed is 498.6 j. Which is the gas?
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