When a 1.0560 g benzoic acid sample was burned in a bomb calorimeter to establish the calorimeter constant, a temperature rise of 2.862 k was measured near 298k. under similar conditions, a temperature rise of 2.416 k was measured when a 0.5863 g naphthalene sample was burned. determine the calorimeter constant (in units of kj/k) and the standard enthalpy of combustion for naphthalene at 298k. if we make the assumption that ∆h ≈∆u, is the ∆chº value obtained from this experim

ΔcH

Explanation:

Hello,

In this case, naphthalene has a Cp=156.1J/(mol*K) and the following equation must be applied to find the enthalpy of combustion (negative since it is about an outgoing form of energy) considering the given assumption (∆H ≈∆U)

ΔcH=Cp*ΔT

ΔcH

For the calorimeter constant, we develop:

Best regards.

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.

answer:

the answer is 6 valence electrons.

explanation:

valence is the # of electrons on the outer most shell of an atom.

oxygen has 6.

although, the valency of oxygen is 2, because it only needs to make 2 covalent bonds, or gain 2 electrons, to achieve the stable octet configuration of a noble gas.

that's it!

if you need further assistance, let me know: )

~ trueboss72