Practice Grams Grams Conversions. 1) How many grams of CO can be made from 180.255 Balanced Chemical Equation : 1 SiO, +3 C 1 SiC +2 CO grams of SiO,? Step 2: Given 180.255 grams of SiO2, Use the molar mass to convert into Moles SiO2. Known Info [Туре 1 [Type ] Step 3: Use the coefficients of a balanced chemical equation to find the mole ratio Mole ratio : [Type] [Type ] (This is conversion factor for step 4) Step 4 Use the mole ratio to convert into Moles of CO Result from Step 2 [Type] [Type ] Moles CO %3D 1 Step 5: Convert from moles into grams of CO. Result from Step 4 [Туре] [Турe 1 1

Practice Grams Grams Conversions. 1) How many grams of CO can be made from 180.255 Balanced Chemical Equation : 1 SiO, +3 C 1 SiC +2 CO grams of SiO,? Step 2: Given 180.255 grams of SiO2, Use the molar mass to convert into Moles SiO2. Known Info [Туре 1 [Type ] Step 3: Use the coefficients of a balanced chemical equation to find the mole ratio Mole ratio : [Type] [Type ] (This is conversion factor for step 4) Step 4 Use the mole ratio to convert into Moles of CO Result from Step 2 [Type] [Type ] Moles CO %3D 1 Step 5: Convert from moles into grams of CO. Result from Step 4 [Туре] [Турe 1 1

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

Section: Chapter Questions

Problem 17STP

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Consider the equation: 2A+B5C. If 10.0 g of A reacts with 5.00 g of B. how is the limiting reactant determined? Choose the best answer and explain. l type='a'> Choose the reactant with the smallest coefficient in the balanced chemical equation. So in this case, the limiting reactant is B. Choose the reactant with the smallest mass given. So in this case, the limiting reactant is The mass of each reactant must be converted to moles and then compared to the ratios in the balanced chemical equation. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must he converted to moles first. The reactant with the fewest moles present is the limiting reactant. So in this case, the limiting reactant cannot be determined without the molar masses of A and B. The mass of each reactant must be divided by their coefficients in the balanced chemical equation, and the smallest number present is the limiting reactant. So in this case, there is no limiting reactant because A and B arc used up perfectly.
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.
Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): :math>C5H12(l)+O2(g)CO2(g)+H2O(l) a 20.4-gram sample of pentane is burned in excess oxygen, what mass of water can be produced, assuming 100% yield?
Solid calcium carbide (CaC2)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. l type='a'> Write the balanced equation for the reaction that is (occurring. including all phases. If a 100.0-g sample of calcium carbide (CaC2)is initially reacted with 50.0 g of water, which reactant is limiting? Prove that mass is conserved for the reactant amounts used in pan b.
Explain how one determines which reactant in a process is the limiting reactant. Does this depend only on the masses of the reactant present? Give an example of how to determine the limiting reactant by using a Before-Change-After (RCA) table with a balanced chemical equation and reactant starling amounts.
For each of the following unbalanced chemical equations, suppose exactly 5.0 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected, assuming that the limiting reactant is completely consumed. msp;Na(s)+Br2(l)NaBr(s) msp;Zn(s)+CuSO4(aq)ZnSO4(aq)+Cu(s) msp;NH4Cl(aq)+NaOH(aq)NH3(g)+H2O(l)+NaCl(aq) msp;Fe2O3(s)+CO(g)Fe(s)+CO2(g)
For each of the following balanced chemical equations, calculate how many grams of the product(s) would be produced by complete reaction of 0.125 mole of the first reactant. msp;AgNO3(aq)+LiOH(aq)AgOH(s)+LiNO3(aq) msp;Al2(SO4)3(aq)+3CaCl2(aq)2AlCl3(aq)+3CaSO4(s) msp;CaCO3(s)+2HCl(aq)CaCl2(aq)+CO2(g)+H2O(l) msp;2C4H10(g)+13O2(g)8CO2(g)+10H2O(g)
The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A at-oms are shown in blue and B atoms in white). The box on the left represents the box on the right shows what is left once the reaction has gone to completion. Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Citric acid, C6H5CH3, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger . The equation representing this reaction is C12H22O11+H2O+3O22C6H8O7+4H2O What mass of citric acid is produced from exactly 1 metric ton (1.000103kg) of sucrose if the yield is 92.30%?
itamin B12 , cyancobalamin, is essential for human nutrition. Its molecular formula is C63H88CoN14O14P . A lack of this vita min in the diet can lead to anemia. Cyanocohalamin is the form of the vitamin found in vitamin supplements. l type='a'> What is the molar mass of cyanocobalamin to two decimal places? How many moles of cyanocohalamin molecules are present in 250 mg of cyanocobalamin? What is the mass of 0.60 mole of cyanocobalamin? How many atoms of hydrogen are in 1 .0 mole of cyanocobalamin? What is the mass of 1.0107 molecules of cyanocobalamin? What is the mass (in grams) of one molecule of cyanocobalamin?
A compound is composed of the elements, carbon, hydrogen, and fluorine only. Combustion of the compound produces CO2, H2O, and HFC?H?F? + O2 ➝ CO2 + H2O + HFCombustion of a 8.000 g sample of the compound produces the products shown in the table below. Product Mass (grams) CO2 15.182 H2O 3.625 HF 3.451 Determine the empirical formula for the compound. [Enter the subscript values for each element in the empirical formula. If an element has a subscript of 1, enter 1]Empirical Formula: C_H_F_
Ammonia can be produced using the Haber process, depicted below (not balanced): H2 (g) + N2 (g) → NH3 (g) If 16.1 grams of hydrogen gas were reacted with an excess of nitrogen gas and 80.5 grams of ammonia were produced, what would be the percent yield of the reaction? Note: Enter the percentage, NOT the decimal (e.g. if 45.4%, enter 45.4, NOT 0.454)