Hydrogen and oxygen are reacted and the water formed is collected at 25°C, where it has a density of 0.997 g/mL. If 36.8 g of H2 and 168 g of O2 are reacted, how many mL of water will be collected?

3. In a particular reaction 8.60g of dinitrogen trioxide gas (N2O3) was actually produced by reacting 6.85 g of oxygen gas (O2) with excess nitrogen gas (N2). a) Write a balanced chemical equation for the reaction. Be sure to include physical states in the equation. b) Calculate the theoretical yield (in grams) of dinitrogen trioxide. Use dimensional analysis. c) Calculate the % yield of dinitrogen trioxide.

For the following reaction, 11.2 grams of glucose (C6H12O6) are allowed to react with 15.5 grams of oxygen gas. glucose (C6H12O6) + oxygen---> carbon dioxide + water What is the maximum amount of carbon dioxide that can be formed? Mass =___ g What is the FORMULA for the limiting reactant?   What amount of the excess reactant remains after the reaction is complete? Mass =___ g

Gasoline is primarily composed of iso-octane, which has the chemical formula C8H18. When gasoline is burned, the chemical equation is: 2C8H18  +  25O2  --->  16CO2 + 18H2O This means that 2 molecules of iso-octane combine with 25 oxygen molecules to produce 16 carbon dioxide molecules and 18 water molecules. Use of fossil fuels adds CO2, carbon dioxide, to the atmosphere. This human-generated CO2 increases the planetary greenhouse effect, leading to an increase in average land surface temperatures, accumulation of heat in the oceans, and modification of global climate. Part of the problem is that a lot of CO2 is produced per mass of fuel burned. You can see that by looking at the fraction of carbon in iso-octane and carbon dioxide. 1. Calculate the formula masses of iso-octane (C8H18) and carbon dioxide (CO2) 2. What is the percent composition of carbon (C) in C8H18 and CO2?