A 338.4-g sample of an iron (III) oxide, Fe₂O₃ is reacted with 154.5 L (measured at

room temperature) of carbon monoxide, CO as shown by the following equation.

Fe₂O₃(s) + 3CO(g) --> 2Fe(s) + 3CO₂(g)

Determine the volume of CO₂ gas evolved at STP.

A solution containing 0.2 mole fraction of H₂SO₄ has a density of 1.5 g/mL. Calculate the

molarity of H₂SO₄.

An organic compound is found to contains 10.59% of hydrogen, 47.3% of carbon and the balance are oxygen. Determine the empirical formula of the compound

The mass spectrometer analysis shows the isotopic Br-79 and Br-81 are 78.9193 u and 80.9163 u respectively. If the average atomic of Bromine is 79.8092 u, calculate percentage abundances of Br-79

You are given 2.5g of C₂₀H₂₄N₂O₅.Determine the mass of carbon atom in the compound

The equation below is not balanced. In order to have a balanced equation,

using ion-electron method, determine the amount of H₂O(l) present in the

equation. Cr₂O₇²⁻(aq) + H⁺(aq) +NO^2-(aq) → Cr³⁺(aq) + NO³⁻(aq)

Zinc reacts with hydrochloric acid according to the equation below. If 0.05 mole of zinc was added to 0.075 mole of hydrochloric acid, deduce the

amount (in gram) of zinc chloride formed.

Zn(s) + 2HCl(aq)→ ZnCl₂(aq) + H₂(g)

Urea, CO(NH₂)₂ is used as fertilizer. The raw materials for making urea are ammonia and carbon dioxide. When 1.0 mole of ammonia reacts with excess carbon dioxide, 25.6 g of urea are produced. What is the percentage yield of

urea in this reaction?

2NH₃(g) + CO₂(g)→ CO(NH₂)₂(s)+ H₂O(l)

Determine the empirical of hydrocarbon which contains 85.6% of carbon (Ar of C= 12 , H=1)