Mass+to+Mole+Conversion+Practice+(NEW)

1. What quantity is conserved in the reaction shown below? (circle all that apply) 2 HCI + Ca(OH)₂ 2 H₂O + CaCl₂ molecules moles atoms mass (grams)

DIRECTIONS: This time, try to follow the process of calculating what is the required until you can get the CORRECT answer. Masa A Mole A Mole B Mole A Mole B Molar Mass B Molar Mass A Mole A Mole B Propane (CSHA) reacts with Oxygen gas to form Carbon Dioxide and water. f 38 g of water are produced in the reaction, how many moles of CO2 were produced? Write the Corect Equation: Balance the Equation: Then solve, follawing the stoichiometric process and the use of the stoichiometric map.

_________ (Answer) (Units)

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A student mixes magnesium and hydrochloric acid and a chemical reaction occurs, shown in the equation below.                                                     ____ Mg + _____ HCl -------->   _____ H2 + ______ MgCl   1.) How many moles of magnesium would you need for the reaction if you had 2 moles of HCl?   2.)  How many moles of magnesium would you need for the reaction if you had 4 moles of HCl?   3.)  How many moles of hydrogen gas (H2) would be produced if you started with 2 moles of magnesium and 2 moles of hydrochloric acid (HCl)?

A student mixes magnesium and hydrochloric acid and a chemical reaction occurs, shown in the equation below.                                                     ____ Mg + _____ HCl -------->   _____ H2 + ______ MgCl   g.) If you started with 2 moles of magnesium and 6 moles of hydrochloric acid (HCl), which one would be your limiting reactant? Which one would be your excess reactant?   h.)  Using the information from part e, how many moles of hydrogen gas (H2) would be produced if you started with 2 moles of magnesium and 6 moles of hydrochloric acid (HCl)? How many moles of reactant would be leftover?

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When the following equation is balanced, the coefficient of O2 is __________.                 C4H8O(g) + O2 (g) →  CO2(g) + H2O(g)       12     11     8     6     10

The in a balanced equation represent numbers of molecules. In a chemical equation, the are written on the left side of the arrow, and the are written on the right side of the arrow.

QUESTION 2 You will assess the percent yield of the reaction. The percent yield is a measure of how efficiently you ran the reaction. In order to do this we will divide the mass of the isolated product by the mass of possible product and then multiply by 100 to get a percentage. Another way of saying this is the yield divided by the yield, multiplied by 100 to get a percentage.

NH3 (g)  +  HCl(g)  ---------> NH4Cl (s)    How many moles of ammonium chloride would be produced by the complete reaction of .7 moles of ammonia?

Converting between quantities To convert from a given quantity of one reactant or product to the quantity of another reactant or product • First, convert the given quantity to moles. Use molar masses to convert masses to moles, and use Avogadro's number (6.02 x 10 particles per mole) to convert number of particles to moles. • Next, convert moles of the given reactant or product to moles of the desired reactant or product using the coefficients of the balanced chemical equation. For example, in the chemical equation2H2 + O2-2H20the coefficients tell us that 2 mol of H2 reacts with 1 mol of Oz to produce 2 mol of H20. • Finally, convert moles of the desired reactant or product back to the desired units. Again, use molar masses to convert from moles to masses, and use Avogadro's number to convert from moles to number of particles. Reaction of hydrogen and nitrogen to form ammonia Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation 3H2(g) +…

According to the following reaction, how many moles of chlorine gas are necessary to form 0.571 moles iron(III) chloride?iron (s) + chlorine (g) -> iron(III) chloride (s) _____ moles chlorine gas

i don’t understand how to solve