An "ideal" fuel'air mixture in which both the fuel and the oxygen in the air are completely consumed is called the "stoichiometric" mixture. The stoichiometric mixture is usually specified as the ratio of the mass of air to the mass of a particular fuel. For example, if a fuel (for example, natural gas, CH4) required 17.2 kg of air to precisely burn 1 kg of the fuel (that is, all the fuel burned and there was no oxygen left in the air afterwards) then the stoichiometric ratio for that fuel would be 17.2: 1. Calculate the partial pressures of the natural gas and oxygen in the mixture based on the stoichiometric ratio given above at 293.15 K. The volume of the internal combustion engine is considered to be 2.500 L. The mass of the fuel is 160.0 g. Mass fraction of oxygen in air is 23.1%. Molar mass of natural gas is 16.043 g/mol. P natural gas = atm Poxygen=[ atm

What is true for this chemical reaction: CO₂(g) + 4H₂(g) = CH₂(g) + 2H₂O(g)? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a AHxn>0; ASrxn > 0 b C d AHrxn 0 AHrxn < 0; ASrxn < 0 AHxn 0; ASxn < 0

What is the easiest process to get to the result?

Commercial drain cleaners contain sodium hydroxide and aluminum. When water is added to this mixture, the heat that is generated will melt grease and the gas that is created will stir up the particles that are clogging the drain. If the process proceeds according to the following reaction: 2 Al (s) + 2 NaOH (aq) + 6 H2O (l) → 2 NaAl(OH)­4 (aq) + 3 H2 (g)   If you use 5.6 g of Al (s) and excess sodium hydroxide, how many liters of H2 (g) at 742 mm Hg and 22.0 ˚C are produced?

Soda ash (sodium carbonate) is widely used in the manufacture of glass.  Prior to the environmental movement much of it was produced by the following reaction.   CaCO3 + 2 NaCl → Na2CO3 + CaCl2   Unfortunately, the byproduct calcium chloride is of little use and was dumped into rivers, creating a pollution problem.  As a result of the environmental movement, all of these plants closed.  Assume that 125g of calcium carbonate (100.09 g/mol) and 125 g of sodium chloride (58.44 g/mol) are allowed to react.   Determine how many grams of useful sodium carbonate (105.99 g/mol) will be produced.  How many grams of useless calcium chloride (110.98 g/mol) will be produced?  You should also determine how many grams of excess reactants are left (indicate which one is the limiting reactant)

11.08 g of liquid methanol (CH,OH) is burned in excess oxygen gas according to the following reaction: 2 CH3OH(1) + 3 02 (g) → 2 CO2(g) + 4 H20(1)

When aqueous solutions of magnesium chloride (MgCl2) and silver nitrate (AgNO3) are mixed, the products are solid silver chloride and aqueous magnesium nitrate. Write the balanced chemical equation for this reaction. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.)

Consider a small bird of mass 30 g. What is the minimum mass of glucose that it must consume (and burn) to fly up to a branch 10 m above the ground?

Answer the following questions using the stoichiometric calculation in chemistry.

Butane, C4H10C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is   2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l)2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atmatm and 23 ∘C∘C, what is the volume of carbon dioxide formed by the combustion of 2.00 gg of butane?