A 4.65 g sample of an oxide of copper, when heated in a streamof hydrogen produces Cu(s) and 0.585 g H2O.What is the formula for the copper oxide?
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Hydrogen gas is passed over 10.00 g of a hot copper oxide (acompound of copper and oxygen). The copper oxide is reactedcompletely to copper metal (Cu(s)) and 1.26 g of water is alsoformed.I believe the percent copper and percent oxygen by mass in thecopper oxide is 88.79% and 8.88% respectively.b. Find the empirical formula of the copper oxide.
Given that 0.160g copper when heated in oxygen becomes copper oxide of mass 0.200g, determine the formula of copper oxide (AW: O 16, Cu 63.6)
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When copper(II) oxide is heated in hydrogen gas, the following reaction takes place.
A copper rod coated with copper(II) oxide has a mass of 38.72 g. The rod is heated and made to react with 5.67 L of hydrogen gas, whose density at the conditions of the experiment is 0.0519 g/L.
(a) How many grams of CuO were converted to Cu?
(b) What is the mass of the copper after all the hydrogen is consumed? (Assume that CuO is converted only to Cu.)