Question: A 2 077 g sample of an element which has an
A 2.077 g sample of an element, which has an atomic mass between 40 and 55, reacts with oxygen to form 3.708 g of an oxide. Determine the formula of the oxide and identify the element.
Answer to relevant QuestionsAmmonia reacts with O2 to form either NO(g) or NO2(g) according to these unbalanced equations: NH3(g) + O2(g) → NO(g) + H2O(g) NH3(g) + O2(g) → NO2(g) + H2O(g) In a certain experiment, 2.00 moles of NH3(g) and 10.00 ...A compound containing only C, H, and N yields the following data. i. Complete combustion of 35.0 mg of the compound produced 33.5 mg of CO2 and 41.1 mg of H2O. ii. A 65.2-mg sample of the compound was analyzed for nitrogen ...Hydrogen cyanide gas is commercially prepared by the reaction of methane [CH4(g)], ammonia [NH3(g)], and oxygen [O2(g)] at a high temperature. The other product is gaseous water. a. Write a balanced chemical equation for the ...A chemist weighed out 5.14 g of a mixture containing unknown amounts of BaO(s) and CaO(s) and placed the sample in a 1.50-L flask containing CO2(g) at 30.0oC and 750. torr. After the reaction to form BaCO3(s) and CaCO3(s) ...You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/ L. Assume ideal behavior and constant temperature. a. What is the ...
Post your question