magnesium and iron nitrate react in a single displacement reaction. what mass of magnesium is needed to completely react 265 grams of iron nitrate (iii)

When chemists work with solid materials, we simply weigh out amounts of solid reagents and calculate mole amounts when thinking about stoichiometry. However, when we dissolve a solid (also known as a solute) in a solvent to form a solution, the solute becomes evenly distributed throughout the solution and we need to know how many moles of solute are present in a particular volume of solution.   A solution is created by dissolving 12.5 grams of ammonium chloride in enough water to make 295 mL of solution. How many moles of ammonium chloride are present in the resulting solution?   When thinking about the amount of solute present in a solution, chemists report the concentration or molarity of the solution. Molarity is calculated as moles of solute per liter of solution. What is the molarity of the solution described above?   To carry out a particular reaction, you determine that you need 0.0500 moles of ammonium chloride. What volume of the solution described above will you need to…

1.0 chem q

if a solution containing 53.927 g of mercury (II) chlorate is allowed to react completely with a solution containing 17.796 g of sodium dichromate how many grams of solid precipitate will form? How many grams of the reactant in excess will remain after the reaction?

In a double replacement reaction, 1.214 g of tin(ii) fluoride react with sodium phosphate to form a precipitate. If the tin (ii) phosphate precipitate weighs 1.078 g, what is the percent yield?

4. When a solution containing 15.0 g of lead (II) nitrate and a solution containing 15.0 g of potassium iodide are mixed, a yellow precipitate of lead (II) iodide is formed. If 6.68 g of the precipitate are formed, what is the percent yield for the reaction?

According to the following reaction, how many grams of ammonia will be formed upon the complete reaction of 23.1 grams of hydrogen gas with excess nitrogen gas?nitrogen (g) + hydrogen (g) ammonia (g)

Consider the following data gathered in the "Molar Mass of a Gas" experiment.   * Mass of the empty reaction test tube: _____27.54_____ g * Mass of the test tube and MnO2 used in the reaction: ____28.04___ g * Mass of the test tube, KClO3 (MM = 122.55 g/mol) and MnO2 used in the reaction: ____29.31___ g * Mass of the test tube and its contents after the reaction: ____ (2.87x10^1) _____ g * Volume of the bubble of oxygen generated in the experiment: ___356___ mL * Atmospheric pressure in the lab: ______766.06______ mm Hg * Vapor pressure at reaction temperature: _____18.6_____ m Hg   Calculate the mass of oxygen generated in the reaction

What is the total mass of products formed with 16 grams of methane (CH4) is burned with excess oxygen?

1.13 g H₂ is allowed to react with 10.3 g N₂, producing 2.13 g NH3.  What is the theoretical yield in grams for this reaction under the given conditions and the percent yield?