Suppose 13.4 g of oxygen(O 2 , 32.0 g/mol) is heated at constant atmosphericpres

Question

Suppose 13.4 g of oxygen(O2, 32.0 g/mol) is heated at constant atmosphericpressure from 18.0°C to140°C. (a) How many moles of oxygen are present?
1 mol

(b) How much energy is transferred to the oxygen as heat? (Themolecules rotate but do not oscillate.)
2 J

(c) What fraction of the heat is used to raise the internal energyof the oxygen?
3 (a) How many moles of oxygen are present?
1 mol

(b) How much energy is transferred to the oxygen as heat? (Themolecules rotate but do not oscillate.)
2 J

(c) What fraction of the heat is used to raise the internal energyof the oxygen?
3

Explanation / Answer

(b) This is a constantpressure process with a diatomic gas, We note that a changeof Kelvin temperature is numerically the same as a

change of Celsiusdegrees.

Q = n CpT = n ( 7/2 R ) T = ( 0.418 mol ) ( 7/2 ) ( 8.31J/mol.K ) ( 122 K ) = ----- J

(c) We could compute a value ofEint from Eq. 19-45 and divideby the result from part (b), or perform this manipulationalgebraically to show the generality of this answer (thatis, manyfactors will be seen to cancel). We illustrate the latterapproach:

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