Calculate the mass in grams of CuO needed to prepare the minimum number of moles of product as noted below.?

The experiment calls for preparing one of two salts, either copper(ii) sulfate or potassium aluminum sulfate. The instructions for the copper(ii) sulfate preparation give a target of between 0.010 and 0.025 moles of the copper(ii) sulfate product. The instructions also specify to use an excess of sulfuric acid... show more The experiment calls for preparing one of two salts, either copper(ii) sulfate or potassium aluminum sulfate. The instructions for the copper(ii) sulfate preparation give a target of between 0.010 and 0.025 moles of the copper(ii) sulfate product. The instructions also specify to use an excess of sulfuric acid but not more than 5 The experiment calls for preparing one of two salts, either copper(ii) sulfate or potassium aluminum sulfate. The instructions for the copper(ii) sulfate preparation give a target of between 0.010 and 0.025 moles of the copper(ii) sulfate product. The instructions also specify to use an excess of sulfuric acid but not more than 5 times the amount required by the balanced equation. Calculate the mass in grams of CuO needed to prepare the minimum number of moles of product as noted above. Report this mass of CuO to two significant figures. Do not include units in the answer box.

CuO(s) + H2SO4(aq) --> CuSO4(aq) + H2O(l)
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