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)

_________ (Answer) (Units)

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3 Na + FeCl3 →Fe +3 NaCl Which of the following statements correctly explains the steps needed to calculate the amount of moles of Fe produced from 3 moles of FeCl3?   Question 7 options:   The first conversion is mole ratio and then use molar mass   The first conversion is molar mass and then use mole ratio   Use molar mass only   Use mole ratio only

Question 5 of 11 Submit Consider the balanced chemical reaction below. How many grams of carbon monoxide are required to react with 6.4 g of iron(III) oxide? Fe,0,(s) + 3 CO(g) → 2 Fe(s) + 3 C0,(g) 1 2 NEXT > Based on your knowledge of stoichiometry, set up the table below to determine the minimum number of moles of CO required to react with the Fe,O, and then determine the amounts after the reaction goes to completion. Fe,O,(s) 3 Co(g) 2 Fe(s) 3 cO,(9) + Before (mol) Change (mol) After (mol) 2 RESET 6.4 -6.4 3.2 -3.2 0.020 -0.020 0.040 -0.040 0.060 -0.060 0.080 -0.080 0.12 -0.12 0.089 -0.089 0.27 -0.27 +

HCl+NH3 >>>>> NH4 Cl 0.134 moles of HCl are reacted with 0.211 moles of NH3 When 0.134 moles of HCl reacts with 0.211 moles of NH3, how much NH3 is consumed?

Part 3- Stoichiometry Calculations 1. How many molecules of chlorine are needed to react with 5.6 g of iron to form iron (III) chloride? 2. 90.0 g of FeCl3 reacts with 52.0 g of H2S. a) Write the balanced chemical equation for this reaction: a) What is the limiting reactant? b) What is the mass of HCl produced? c) What mass of excess reactant remains after the reaction? 9. Given the heat of reaction for the combustion of propane: -2220KJ/mol a) Write the heat of reaction equation for the combustion of propane (C3H8). b) Calculate the heat of reaction for the combustion of propane when 33.0g of CO2 is produced.

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.

Question 10 of 10 Consider the balanced chemical reaction below. What is the maximum number of grams of Ag that can be produced if 0.57Ctmol of Zn and 0.691 mol of Ag20 react? Zn(s) + Ag,0(s) → ZnO(s) + 2 Ag(s) 2 NEXT Based on your knowledge of stoichiometry, set up the table below to determine the amounts of each reactant and product after the reaction goes to completion. Zn(s) Ag20(s) ZnO(s) 2 Ag(s) + Before (mol) 0.691 0.570 Change (mol) 0.570 0.570 0.570 1.140 0.570 1.140 0.121 After (mol) Incorrect, 1 attempt remaining In this problem, the Change in moles for Zn is incorrect. Make sure you have identified the limiting reactant in this reaction (the species that will have 0 moles remaining after the reaction). Once you have identified the limiting reactant, use stoichiometry along with the given balanced Goutucourses are you naving amIcURy Math 153 OCT tv 13

When the following equation is properly balanced, the coefficient in front of HCl is                  .                  C3H8 (g) +         Cl2 (g)   ➞         C3H6Cl2 (g) +          HCl (g)         1     2     4     6     5

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) +…