1. The problem statement, all variables and given/known data Calculate what mass of carbon you would need to reduce 15.9g of copper(II) oxide to copper by the reaction: CuO(s) + C(s) [tex]\rightarrow[/tex] Cu(s) + CO(s) 2. Relevant equations n = m / ar (number of moles = mass / relative atomic mass) If you know any more, it would be really useful for me though ;) . 3. The attempt at a solution Ar(Cu) = 63.5 Ar(O) = 16.0 Ar(C) = 12.0 CuO = 1 / (63.5 + 16.0) = 79.5g C = 1 / (12.0) = 12.0g 79.5 / 79.5 * 15.9 = 15.9g of CuO 12.0 / 79.5 * 15.9 = 2.4g of C Basically, I divided the mass of CuO by the mass of CuO and multiplied by 15.9 to get 15.9g (as in the question). Then, I applied the same equation to C by dividing the mass of C by 79.5 and then multiplying by 15.9 to get 2.4g, which is my answer. Is this correct?