copper has a $delta h_{fus}=13.0 kj/mol$. what mass of copper releases 112.4 kj of heat as it freezes? use…

copper has a $delta h_{fus}=13.0 kj/mol$. what mass of copper releases 112.4 kj of heat as it freezes? use $q = ndelta h$.\n9.42 g\n6.75 g\n549 g\n1590 g

copper has a $delta h_{fus}=13.0 kj/mol$. what mass of copper releases 112.4 kj of heat as it freezes? use $q = ndelta h$.\n9.42 g\n6.75 g\n549 g\n1590 g

Answer

Explanation:

Step1: Calculate the number of moles (n)

Given $q = n\Delta H$, we can solve for $n$. Rearranging the formula gives $n=\frac{q}{\Delta H}$. Substituting $q = 112.4\ kJ$ and $\Delta H=13.0\ kJ/mol$, we have $n=\frac{112.4\ kJ}{13.0\ kJ/mol}=8.646\ mol$.

Step2: Calculate the mass of copper

The molar - mass of copper ($Cu$) is $M = 63.55\ g/mol$. Using the formula $m=nM$, where $n = 8.646\ mol$ and $M = 63.55\ g/mol$, we get $m=8.646\ mol\times63.55\ g/mol = 549\ g$.

Answer:

549 g