Here the example says, if 15.7 grams of silver raises its temperature by 17.2 degrees Celsius when it absorbs 6,845.5 joules, what is its molar heat capacity? So, molar heat capacity uses capital C. It's equal to heat, which is \( q \) divided by moles \( n \) times change in temperature \(\Delta T\). In the question, it says that we're absorbing this much energy. That means that that's a positive \( q \). So that's positive 6,845.5 joules.

Next, we need moles, and we already have the change in temperature. They said that the temperature was risen by 17.2 degrees Celsius. So that's already our change in temperature. We need moles. We have here 15.7 grams of silver, which is \( g \). We have to change that to moles, so one mole of silver weighs 107.87 grams according to the periodic table. So that comes out to be 0.145548 moles of silver. Take those moles and plug it in. So when we do that, that's going to give me my molar heat capacity as 2,734.45 joules over moles times degrees Celsius. If we look at our values, this has 3 significant figures and this has 3 significant figures, so I could change this to \( 2.73 \times 10^3 \) joules over moles times degrees Celsius. So that would be the molar heat capacity for silver under these conditions.