Homework Answers
Balanced equation:
2 C7H14 + 21 O2 ===> 14
CO2 + 14 H2O
Reaction type: combustion
3 Ca(OH)2 + 2
H3PO4 =
Ca3(PO4)2 + 6
H2O
Reaction type: double replacement
5H2O2 + 2KMnO4 + 3H2SO4 ===> 5O2 + 2MnSO4 + K2SO4 + 8H2O
Redoc reaction
Quesion 2
Balanced equation:
2 NO + 5 H2 ===> 2 NH3 + 2
H2O
Reaction type: double replacement
86.3 gm of NO = 86.3 /30 = 2.876 Moles
25.6 gm of H2 = 25.6 / 2.016 = 12.69 Moles
Limiting regent is NO
Molesk of NH3 to be produced = 2.876 Moles
Mass of NH3 produced (Thoretical yield) = 2.876 x 17.03 = 48.98 gm
Question 3
Balanced equation:
TiO2 + 2 C ===> 2 CO + Ti
Reaction type: single replacement
28.6 Kg of C = 28.6 x 103 / 12.01 = 2381.2 Moles
88.2 Kg of TiO2 = 88.2 / 79.86 = 1104.3 Moles
Limiting reagent is TiO2
Moles of Ti Produced = 1104.35 Moles
Mass of TiO2 produced (Thoretical Yeld) = 1104.35 x 47.86 / 1000 = 52.862 Kg
Percentage yield = 42.8 x 100 / 52.862 = 80.965 %
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PLTL Worksheet Spring 2018 Chapter 3 & 11 Nameah laicr 1. Balance the following equations: 4...
Excess Reactant Examples: 12. Recall from Example 10 that we can extract titanium metal from its...
Excess Reactant Examples: 12. Recall from Example 10 that we can extract titanium metal from its oxide according to the following balanced equation: TiO:(s) + 2 C(s)_ Ti(s) + 2 CO(g) Recall further that in a reaction mixture containing 28.6 kg of C and 88.2 kg of TiOz, TiO2 is the limiting reactant. Calculate the mass of the reactant in excess (which is carbon) that remains after the reaction has gone to completion.
Q.1. Ammonia, NH3, can be synthesized by the reaction: 2 NO(g) + 5 H2(g) →→ 2...
Q.1. Ammonia, NH3, can be synthesized by the reaction: 2 NO(g) + 5 H2(g) →→ 2 NH3(g) + 2 H2O(g) Starting with 86.3 g NO and 25.6 g H2, find the theoretical yield of ammonia in grams. Ans.
D. Complete the following stoichiometry problems. Show ALL of your work to receive full credit. Equations...
D. Complete the following stoichiometry problems. Show ALL of your work to receive full credit. Equations and mole-to-mole relationships 21. For the following reaction: 4Cr(s) + 302(g) → 2Cr2O3(s) a. How many moles of oxygen (O2) would react with 0.35 moles of chromium (Cr)? b. Starting with 10.4g of Oz, how many moles of Cr203 can be produced: c. How many grams of Cr metal would be needed to produce 38.2g of chromium (III) oxide? 22. Sulfuric acid (H2SO4) is...
Question 17 (4 points) Verify the following chemical equation is balanced TiO2 + 3 C →...
Question 17 (4 points) Verify the following chemical equation is balanced TiO2 + 3 C → Ti + 2 CO If you begin with 88.2 kilograms of TiO2, how many kilograms of Ti can you make? 0 26.4 kg of Ti 52.9 kg of Ti 47.8 kg of Ti 26.4 g of Ti
1. Calculate the number of moles in each sample. a. 15.7 g CCl b. 1.8 x...
1. Calculate the number of moles in each sample. a. 15.7 g CCl b. 1.8 x 1021 formula units of NaC 2. Calculate the number of grams in each sample 1.23 mol magnesium bromide 7.310 x 1025 molecules of H202 a. b. 3. Calculate the mass percent of H in each of the following compounds. C2H2 C2HsCI a. b. 4. Calculate the empirical formula of each of the following Methy butyrate: 58.80 % C, 9.87 % H, 31.33 % O...
A. Balance the following equations by adding coefficients. Do not leave blank spaces - use a...
A. Balance the following equations by adding coefficients. Do not leave blank spaces - use a "1" if necessary. Identify the type of reaction in the right column. Balanced Equation Type of Reaction 1. H.As2O7 → _ As2O3 + _H20 2. _N2+_02—_N20 _NaI + _Br2 → _NaBr +_12 PbCrO4 +_HNO3 → __Pb(NO3)2 + __H2CrO4 . _C3H8 +_02 → __CO2 + __H20 TiCl4 + _ Mg → _ MgCl2 + ____Ti CuSO4 +_ KCN → ___Cu(CN)2 +_K2SO4 Ca(ClO3)2 → _ CaCl2...
Name FUL L U Stoichiometry worksheet (Lab) Please complete the following problems during lab. Do all...
Name FUL L U Stoichiometry worksheet (Lab) Please complete the following problems during lab. Do all of your work on a separate sheet of paper. Show all of your work for full credit and circle your final answer. 1) How many moles of CO2 are produced when 2.5 moles of O2 react according to the following equation? C3H8 (8) +502 (8) ► 3002 (8) + 4H20 (8) 2) In the reaction 2 C(s) + O2(g) 66.0 g of carbon monoxide?...
4. [5 points) Write and balance the following equation: solid lead sulfide reacts with ozone gas...
4. [5 points) Write and balance the following equation: solid lead sulfide reacts with ozone gas (O3) to produce solid lead sulfate and oxygen gas. 5. (10 points) The final stage in refining the metal lead (Pb) is to react lead(II) oxide with carbon, producing lead and carbon dioxide. If 225 g Pbo reacts with 10.0 g C: a. Write the balanced equation for this reaction. b. What is the limiting reactant? c. What is the theoretical yield?
Exercises lI: Stoichiometry and limiting reagents, theoretical yield and percent yield 1. Given the following reaction...
Exercises lI: Stoichiometry and limiting reagents, theoretical yield and percent yield 1. Given the following reaction N2(g) +3H2(g)2NH3(g) (a) How many number of moles of ammonia can be formed from 0.25 moles of N, gas? (b) How many moles of H2 are needed to react with 0.25 moles of N2 gas? O If you begin with a gas mixture that contains 2.00 moles of N2 gas, and 3.0 moles of H2 gas, at the end of reaction, which reactant is...
L. Sy Short Answer (4 questions, 60 points total) 1. In the commercial production of the element arsenic, arsenic I...
L. Sy Short Answer (4 questions, 60 points total) 1. In the commercial production of the element arsenic, arsenic II)oxide (197.84 g/mol)) is heated with carbon, which reduces the oxide to the metal according to the following equation: 2As:0, +30 - 400,- 4s (20 points total) a 18 8.87g of As 0,(197.84 g/mol) is reacted in the presence of excess carbon, what is the theoretical yield of As? b. If 6.33 g of As (74.92 g/mol) is actually produced, what...
Excess Reactant Examples: 12. Recall from Example 10 that we can extract titanium metal from its oxide according to the following balanced equation: TiO:(s) + 2 C(s)_ Ti(s) + 2 CO(g) Recall further that in a reaction mixture containing 28.6 kg of C and 88.2 kg of TiOz, TiO2 is the limiting reactant. Calculate the mass of the reactant in excess (which is carbon) that remains after the reaction has gone to completion.
Q.1. Ammonia, NH3, can be synthesized by the reaction: 2 NO(g) + 5 H2(g) →→ 2 NH3(g) + 2 H2O(g) Starting with 86.3 g NO and 25.6 g H2, find the theoretical yield of ammonia in grams. Ans.
D. Complete the following stoichiometry problems. Show ALL of your work to receive full credit. Equations and mole-to-mole relationships 21. For the following reaction: 4Cr(s) + 302(g) → 2Cr2O3(s) a. How many moles of oxygen (O2) would react with 0.35 moles of chromium (Cr)? b. Starting with 10.4g of Oz, how many moles of Cr203 can be produced: c. How many grams of Cr metal would be needed to produce 38.2g of chromium (III) oxide? 22. Sulfuric acid (H2SO4) is...
Question 17 (4 points) Verify the following chemical equation is balanced TiO2 + 3 C → Ti + 2 CO If you begin with 88.2 kilograms of TiO2, how many kilograms of Ti can you make? 0 26.4 kg of Ti 52.9 kg of Ti 47.8 kg of Ti 26.4 g of Ti
1. Calculate the number of moles in each sample. a. 15.7 g CCl b. 1.8 x 1021 formula units of NaC 2. Calculate the number of grams in each sample 1.23 mol magnesium bromide 7.310 x 1025 molecules of H202 a. b. 3. Calculate the mass percent of H in each of the following compounds. C2H2 C2HsCI a. b. 4. Calculate the empirical formula of each of the following Methy butyrate: 58.80 % C, 9.87 % H, 31.33 % O...
A. Balance the following equations by adding coefficients. Do not leave blank spaces - use a "1" if necessary. Identify the type of reaction in the right column. Balanced Equation Type of Reaction 1. H.As2O7 → _ As2O3 + _H20 2. _N2+_02—_N20 _NaI + _Br2 → _NaBr +_12 PbCrO4 +_HNO3 → __Pb(NO3)2 + __H2CrO4 . _C3H8 +_02 → __CO2 + __H20 TiCl4 + _ Mg → _ MgCl2 + ____Ti CuSO4 +_ KCN → ___Cu(CN)2 +_K2SO4 Ca(ClO3)2 → _ CaCl2...
Name FUL L U Stoichiometry worksheet (Lab) Please complete the following problems during lab. Do all of your work on a separate sheet of paper. Show all of your work for full credit and circle your final answer. 1) How many moles of CO2 are produced when 2.5 moles of O2 react according to the following equation? C3H8 (8) +502 (8) ► 3002 (8) + 4H20 (8) 2) In the reaction 2 C(s) + O2(g) 66.0 g of carbon monoxide?...
4. [5 points) Write and balance the following equation: solid lead sulfide reacts with ozone gas (O3) to produce solid lead sulfate and oxygen gas. 5. (10 points) The final stage in refining the metal lead (Pb) is to react lead(II) oxide with carbon, producing lead and carbon dioxide. If 225 g Pbo reacts with 10.0 g C: a. Write the balanced equation for this reaction. b. What is the limiting reactant? c. What is the theoretical yield?
Exercises lI: Stoichiometry and limiting reagents, theoretical yield and percent yield 1. Given the following reaction N2(g) +3H2(g)2NH3(g) (a) How many number of moles of ammonia can be formed from 0.25 moles of N, gas? (b) How many moles of H2 are needed to react with 0.25 moles of N2 gas? O If you begin with a gas mixture that contains 2.00 moles of N2 gas, and 3.0 moles of H2 gas, at the end of reaction, which reactant is...
L. Sy Short Answer (4 questions, 60 points total) 1. In the commercial production of the element arsenic, arsenic II)oxide (197.84 g/mol)) is heated with carbon, which reduces the oxide to the metal according to the following equation: 2As:0, +30 - 400,- 4s (20 points total) a 18 8.87g of As 0,(197.84 g/mol) is reacted in the presence of excess carbon, what is the theoretical yield of As? b. If 6.33 g of As (74.92 g/mol) is actually produced, what...
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