What mass of K is found in 60.3 g of K3PO4? Enter your answer accurate to three significant figures. Use an appropriate symbol (abbreviation) for the units. Molar masses (in g mol-¹): O, 16.00 Number Units P, 30.97 K, 39.10

Dr. Bunsen Honeydew determined the empirical formula for tungsten oxide (WxOy). To do so, Dr. Honeydew heated 5.47 g tungsten with oxygen in a crucible and formed 6.18 g of tungsten oxide.  W(s) + O2(g) → WxOy(s)  How many moles of tungsten are in the compound? Express your answer to three significant figures. How many moles of oxygen are in the compound? Express your answer to three significant figures. What is the empirical formula of the tungsten oxide? All one quection

1212

N2(g) + 3H2(g) → 2NH3(g) What mass of ammonia (formula: NH3), in grams, would be produced if 525 mg of H2(g) was reacted with an excess of N2(g)?

What is the mass of 3.5 x 10^-3 molecules of copper (II) carbonate? Use correct significant figures and units.

Home-Grown Example: Calculation of Mass-Related Concentrations (a) A solution is made by dissolving 1.675 mg of sucrose (C₁2H22011) in 0.01091 g of water. What is the mass percentage of each component of the solution? (b) A 1762-kg sample of groundwater was found to contain 2.443 µg of Fe²+. What is the concentration of Fe²+ in parts per billion?

[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant.   b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.

True or False? One mole of molecular O2 = 6.02 x 1023 O2 molecules. Mass of O2 in 100g of CO2 = (32.0g ÷0g) x 100 = 72.7 O2

If 31.0 g of MgSO4⋅7H2O is thoroughly heated, what mass of anhydrous magnesium sulfate will remain? Express your answer to three significant figures and include the appropriate units.

You have 2.97 × 10^25 molecules of water. Find the volume of this in milliliters. Water has a molar mass of 18.01528 grams per mole and a density of 1 gram per milliliter. Avogadro's number is always 6.022 × 10^23 molecules per mole. Round to two decimal places.