2CH₃CHO + 5O₂ --> 4CO₂ + 4H₂O

The equation indicates that ___ mole(s) of O₂ are required for each mole of CH₃CHO.

What is the total mass of products formed when 16 g of CH₄ is burned with excess oxygen?

C₃H₈ + 5O₂ --> 3CO₂ + 4H₂O

Then equation indicates that ____ moles of O₂ are required for each mole of C₃H₈.

Balance the following equation with the smallest whole number coefficients possible. Select the number that is the sum of the coefficients in the balanced equation.

KClO₃ --> KCl + O₂

Calculate the mass of hydrogen formed when 27 g of aluminum reacts with excess hydrochloric acid according to the balanced equation below.

2 Al + 6 HCl --> 2 AlCl₃ + 3 H₂

How many grams of nitric acid can be prepared from the reaction of 138 g of NO₂ with 54.0 g H₂O according to the equation below?

3NO₂ + H₂O --> 2HNO₃ + NO

Which of the following is true?

I. The molar mass of CaCO₃ is 100.1 g/mol.

II. 50 g of CaCO₃ contains 9 X 10²³ oxygen atoms.

III. A 200 g sample of CaCO₃ contains 2 moles of CaCO₃.

How many grams of water will be formed when 32.0 g hydrogen is allowed to react with 16.0 g of oxygen according to: 2 H₂ + O₂ --> 2 H₂O?

A given sample of some hydrocarbon is burned completely and it produces 0.44 g of CO₂ and 0.27 g of H₂O. Determine the empirical formula of the compound.

Given that there are two naturally occurring isotopes of gallium, ⁶⁹Ga and ⁷¹Ga, the natural abundance of the ⁷¹Ga isotope must be approximately

In which of the following compounds is the mass ratio of element X to oxygen closest to 2.5 to 1? (The molar mass of X is 40.0 g/mol)