The specific heat capacity of copper is 0.385 J/(gK). If 353 J of heat are added to 3.6 moles of copper at 283 K, what is the final temperature of the sample of copper?

287K

Explanation:

To find the increasing in temperature for the sample of copper we must use the equation:

Q = m*C*ΔT

Q is the heat added (353J)

m is the mass of copper (3.6mol * (63.546g / mol) = 228.8g

C is specific heat (0.385J/(gK))

And ΔT is the increasing in temperature.

Solving for ΔT:

Q / m*C = ΔT

353J /228.8g*0.385J/(gK) = 4.0K

That means the final temperature of copper is:

283K + 4K =

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

2b2t

explanation:

2b2t