Write the conversion factors in the order you would use them to determine correctly each of the following quantities in a sample of 2.0  10 24 molecules of ethane (C 2 H 6 ). The molar mass of ethane is 30.08 g/mol.

The mass of 2.21 x 1040 atoms of iron (molar mass = 55.845 g/mol) is 2.78 x 104 g. 2.05 x 102 g 30.97 g. O 6.22 x 103g O 112 × 10-2 g.

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

Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s) + 3C12(g)-> 2AICI3(s) What is the maximum mass of aluminum chloride that can be formed when reacting 34.0 g of aluminum with 39.0 g of chlorine? Express your answer to three significant figures and include the appropriate units.

Convert 3.45 × 1018 molecules of OF2 to grams. Convert the 15.2 moles of NH4Cl to grams. Convert the 85.0 g of CO to particles. How many oxygen atoms are in 2.50 moles of C6H12O6? Calculate the molar mass of the Pb(CO3)2 (use the periodic table). How many moles of oxygen are in 45.7 moles of potassium nitrate? Convert the 123 g of CaF2 to moles. Convert the 5.62 × 1025 atoms of B to moles.

A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands for a number the student is going to calculate.) Enter the units of the student's answer. (0.19 L) 1 mL 10-³ 146.86 g mol 1.04 mL = ☐ x10 ロ･ロ X I 00

Let us explore a reaction with a limiting reactant. Here, zinc metal is added to a flask containing aqueous HCl, and H2 gas is a product.   The three flasks each contain 0.300 mol of HCl. Zinc is added to each flask in the following quantities: 4.90 g, 9.81 g, 19.6 g.  When the reactants are combined, the  inflates the balloon attached to the flask. The results are as follows: Flask 1: Balloon inflates completely, but some  remains when inflation ceases. Flask 2: Balloon inflates completely. No Zn remains. Flask 3: Balloon does not inflate completely. No Zn remains.   What mass of Zn was added to each flask? Mass = ? g (flask 1) Mass = ? g (flask 2) Mass = ? g (flask 3)

References Use the References to access important values if needed for this question. For the following reaction, 24.3 grams of iron are allowed to react with 27.8 grams of hydrochloric acid. iron(s) + hydrochloric acid (aq) → iron (II) chloride (aq) + hydrogen (g) What is the maximum amount of iron(II) chloride that can be formed? Mass= g What is the FORMULA for the limiting reactant? What amount of the excess reactant remains after the reaction is complete? Mass= g Submit Answer

The formula for alum is KAl(SO4)2  x 12 H2O. All of the atoms in this formula contribute to the molar mass. When you add up all the masses in the formula, the molar mass is 474.39 grams/mole. The molar mass of aluminum is 26.98.   If you started this experiment with 1.063 grams of aluminum foil, what is the theoretical yield      of  Alum? Give your answer to 1 decimal place.  __________________________   The actual yield of alum in the lab was 17.8 grams. What percentage yield is this? Give your       answer to 1 decimal place.  ____________________________

Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) A student used 117.24 g of Ag and obtained 135.49 g of AgNO3, calculate the percent yield of AgNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol