Of which reactant are there the most initial moles? Enter its chemical formula: of which reactant are there the least initial molés? Enter its chemical formula: Which reactant is the limiting reactant? Enter its chemical formula: 0

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:

T Balanced Total Equation (molecular equation) COC2(aq) + AGNO3(aq) Names of reactants and products (write below chemical formulas): Balanced Total Equation (molecular equation)

balance the following unbalanced chemical equation showing the combustion of methane. use 1 for a coefficient of one even though typically no number is written. ______CH4 + ______ O2 --> ______ CO2 + ______ H2O

For the following reaction, 25.3 grams of sulfur dioxide are allowed to react with 5.89 grams of water. sulfur dioxide (g) + water (1) → sulfurous acid (H₂SO3) (g) What is the maximum amount of sulfurous acid (H₂SO3) that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams

Suppose the following chemical reaction can take place in this mixture

For the following reaction, 0.350 moles of carbon (graphite) are mixed with 0.266 moles of oxygen gas. carbon (graphite)(s) + oxygen(g) → carbon dioxide(g) What is the formula for the limiting reagent? What is the maximum amount of carbon dioxide that can be produced? moles

3. Dry ice is the name for solid carbon dioxide. Instead of melting, solid carbon dioxide sublimes according to the equation: When dry ice is added to warm water, heat from the water causes the dry ice to sublime more quickly. The evaporating carbon dioxide produces a dense fog often used to create special effects. In simple dry ice fog machines, dry ice is added to warm water in a Styrofoam cooler. The dry ice produces fog until it evaporates away, or until the water gets too cold to sublime the dry ice quickly enough. A small Styrofoam cooler holds 15.0 Lof water heated to 85 °C. Use standard enthalpies of formation to calculate the mass of dry ice that should be added to the water so that the dry ice completely sublimes away when the water reaches 25 °C. Assume no heat loss to the surroundings. (The AH°; for CO219) is -427.4 kl/mol.)

• Write out the chemical equation for the synthesis of aspirin using ONLY the NAMES of REACTANTS and PRODUCTS!!! (use "+" to separate compounds and "-->" to indicate reactant and product sides of the chemical equation) • Write out the balanced equation for the synthesis of aspirin using chemical formulas: (again use "+" to separate compounds and "-->" to indicate reactant and product sides of the chemical equation, no need for phase labels) • What is the mole ratio of the first reactant and aspirin? What is the mole ratio of the second reactant and aspirin? • Besides aspirin, what its chemical name? The one mentioned in this experiment.

Balance the chemical equation. CS₂ + NH3 H₂S + NH4SCN Assume the coefficient of NHSCN is 1. What is the balanced equation? CS₂ + NH3→H₂S+NHSCN