For the reaction of sodium sulfide with iron(III) chloride below (as an unbalanced reaction - that's how I will almost always give you reactions.  ALWAYS check to see if a reaction is balanced before you use it.  You balanced it in the last question; make sure you have that right before you start calculating!), you have 319.5 kg of sodium sulfide and 502.3 kg of iron(III) chloride available. What mass (in kilograms) of sodium sulfide do you NEED if you're going to reduce  all of the iron(III) chloride you have?   Na2S(s)  +   FeCl3(s)    →   Fe2S3(s)   +  NaCl(s)

Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 4.78 g of magnesium ribbon burns with 7.61 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? охудen O magnesium The reaction goes to completion, but in the process of recovering the product, some of it was lost. The the percent yield for the reaction is 82.8%. How many grams of product are recovered? mass of product recovered: How many grams of the excess reactant remain? Assume the reaction goes to completion. mass of excess reactant:

1) Group 1 metals react almost instantly and violently with water, as a single replacement reaction to produce an aqueous solution of metal hydroxide and hydrogen gas. A sample of solid lithium weighing 84.25 mg is dropped into a beaker containing 50.0 mL of water. Assume the density of water is 0.9988 g/mL. a) Write the balanced equation. b) Calculate the theoretical yield (in grams) of lithium hydroxide. c) Assuming the reaction is complete, and that there is no volume change, what is the concentration (in M) of lithium hydroxide in the solution that results?

% yield = = actual yield / theoretical yield x 100 CuzCOз (ОН)2 ( amounts can all be in mol or all in g) Cuo H20 + CO2 Data and calculations Balance the reaction first Mass (g ) Crucible ( empty) 48.11 Sample 1.00 Crucible ( after heating ) 48.81 Cuo ( actual in g) CuzCOз (ОН)2 molar mass Cuo molar mass Mol Cuo produced ( actual in mol ) Mol sample used

For the following reaction 36.4 grams of sulfuric acid are allowed to react with 40.1 grams of zinc hydroxide. What is the maximum amount of zinc  sulfate that can be formed? What is the formula for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?

A reaction has a theoretical yield of 76.5 grams of a product, and a percent yield of 41.2  %.  What is the actual yield (in g) of this product in this 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?

Balance the following equations (be sure to first convert any chemical names into formulas). Show all steps for balancing or write a brief explanation of your mental process if you were able to balance it in your head. FeCl3 + NaOH → Fe(OH)3 + NaCl P + O2 → P2O5 Lead(II) hydroxide reacts with hydrogen chloride to produce water and lead(II) chloride. Zinc sulfide reacts with aluminum phosphide to produce zinc phosphide and aluminum sulfide.

A student working in a lab, needed to add 1.599 g acetone and 3.2 g of benzaldehyde to a Reaction flask. If the student does not have access to a weighing balance, how would they measure out the reactants ? Provide the name of the equipment/glassware and the final amount that was added to the reaction vial.

When a solution containing 27.2 g of lead (II) nitrate and a solution containing 35.4 g of potassium iodide are mixed, a yellow precipitate of lead (II) iodide is formed. If 13.6 g of the precipitate formed, what was the percent yield for the reaction?  Note: you must write out and balance the equation first.