For the following reaction, 3.65 grams of hydrogen gas are mixed with excess nitrogen gas. The reaction yields 16.8 grams of ammonia. N2 (g) + 3H2 - 2NH3 (g) (1) What is the theoretical yield of ammonia?| grams (2) What is the percent yield for this reaction?

1a) 1b)

7.) A Sample Of 13.3g of Fe₂03 reacts with 16.89 CO со to yield Fe and Co₂. The balanced equation Fe₂O3 (s) + 3 C0g 2 Fe (5) + 300₂ (g) is Which Substance is the limiting reactant? What is the theoretical yield of Fe ? If the actual experimental yield for Fe is 8.41g what is the percent yield of Fe?

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A chemist invents a new combustion analysis instrument that uses less O2(g) which saves money on each analysis. The improvement is that instead of CO2(g) being formed and trapped, CO(g) is formed and trapped. H2O (g) is also formed and trapped when substances that contain hydrogen are analyzed.(a) The chemist places 2.184 g of an unknown compound of carbon and hydrogen in the new analyzer. 4.627 g of CO (g) and 1.795 g of H2O (g) are produced. Find the empirical formula for the compound.(Molar masses (g/mol): CO = 28.0104, H2O = 18.015) (b) Despite the best efforts of the chemist, the molar mass of the compound cannot be determined (using this method). Clearly explain why this prevents the determination of the molecular formula

Tetraphosphorus decoxide reacts with water to produce phosphoric acid. What is the percent yield if 1.464 x 10“ grams of tetraphosphorus decoxide is reacted, 17.57 kilograms of phosphoric acid is actually produced. (Hint: 1 x 10 kg = 1 g) %3D P4010 (g) + 6 H2O (I) ----> 4 H3PO4 (aq) (BALANCED) Substance Molar Mass Tetraphosphorus Decoxide 283.88 g/mol Water 18.02 g/mol Phosphoric Acid 98.00 g/mol

The sample is analyzed and found to contain three elements, C, H and O. A 2.147 g sample of the compounds burns in O2(g) to produce 4.297 g of CO2(g) and 1.757 g of H2O(g). (a) Calculate the moles of C in the sample. (b) Calculate the moles of H in the sample. (c) Calculate the moles of O in the sample. (d) Determine the empirical formula for the compound.

22.0 g of CO​​2 gas and 9.01 g of H​​2O gas are formed from combustion of an unknown hydrocarbon (containing only hydrogen and carbon) in the presence of O​​2 gas. The molar mass of the gas is 84.2 g/mol. What is its molecular formula?

Mg(s) + 2 H2O(l) -> Mg(OH)2(aq) + H2(g) When 11.0g of Mg(s) reacts with excess water to produce 5.75g of Mg(OH)2 , what is the percent yield of the reaction?

When heated, Fe(OH) decomposes into Fe2O3 and water, according to the followingequation:2 Fe(OH)3 (s) > Fe2O3 (s) + 3 H20 (g)If 25.96 g of Fe(OH)3 decomposes, and 11.06 g of Fe2O3g are obtained in the reaction,what is the percent yield of the reaction?