The potassium chlorate (KClO3, 122.55g/mol) in an 0.1862g sample of an explosive was determined by reaction...
The potassium chlorate (KClO3, 122.55g/mol) in an 0.1862g sample of an explosive was determined by reaction with 50.00mL of 0.01162M Fe2+ in the following reaction:
ClO3- + 6Fe2+ + 6H+ --> Cl- + 3H2O + 6Fe3+.
Calculate the percentage of KClO3 in the original sample.
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The potassium chlorate (KClO3, 122.55g/mol) in an 0.1862g sample
of an explosive was determined by reaction...
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s) ....
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s) . The equation for the reaction is 2KClO3⟶2KCl+3O2 Calculate how many grams of O2(g) can be produced from heating 70.4 g KClO3(s) STRATEGY: Convert the mass of KClO3 to moles. Convert the number of moles of KClO3 to the number of moles of O2 . Convert the number of moles of O2 to grams. Step 1: 70.4 g KClO3 is equal to 0.574 mol KClO3...
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s). The...
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s). The equation for the reaction is 2KClO3⟶2KCl+3O2 Calculate how many grams of O2(g) can be produced from heating 98.6 g KClO3(s). mass:
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s). The...
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KClO3(s). The equation for the reaction is 2KClO3⟶2KCl+3O2⟶2KCl+3O2 Calculate how many grams of O2(g) can be produced from heating 48.8 g KClO3(s).
postassium chlorate KClO3 decomposes according to the reaction 2KClO3 -> 2KCl +3O2 if the rate of...
postassium chlorate KClO3 decomposes according to the reaction 2KClO3 -> 2KCl +3O2 if the rate of decomposition of KClO3 at a certain time is determined to be 2.8 x 10 ^-2 mol s-1 what is the rate of formation of KCl at the same time
A sample of iron ore weighing 0.6428g is dissolved in acid, the iron is reduced to...
A sample of iron ore weighing 0.6428g is dissolved in acid, the iron is reduced to Fe2+, and the solution is titrated with 36.30 mL of 0.01753 M K2Cr2O7 solution. The reaction is 6Fe2+ + Cr2O72- +14H+ à 6Fe3+ + 2Cr3+ + 7H2O What is the Percentage of iron (55.85g/mol) in the sample?
Percentage of Oxygen in Potassium Chlorate Introduction: The thermal decomposition of potassium chlorate can be described...
Percentage of Oxygen in Potassium Chlorate Introduction: The thermal decomposition of potassium chlorate can be described by the following equation: 2 KCIO3(s) 2 KCls) + 3 O2(g) Egn 1 (D stands for heating, elevated temperature) In this experiment you will determine the percentage of oxygen in potassium chlorate. You will compare the experimental result with the theoretical percentage calculated from the formula KCIO3. While potassium chlorate decomposes simply by heating, the reaction is very slow. A catalyst is used. Catalyst...
The Fe2+ (55.84555.845 g/mol) content of a 2.028g steel sample dissolved in 50.00mL of an acidic solution was determined...
The Fe2+ (55.84555.845 g/mol) content of a 2.028g steel sample dissolved in 50.00mL of an acidic solution was determined by tiration with a standardized 0.130 M potassium permanganate (KMnO4KMnO4, 158.034 g/mol) solution. The titration required 36.61 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per gram of steel. MnO−4+8H++5Fe2+↽−−⇀Mn2++5Fe3++ concentration: ______________ g Fe/g steel
composition of potassium chlorate questions and problems REPORT FOR EXPERIMENT 9 (continued) B. Qualitative Examination of...
composition of potassium chlorate questions and problems
REPORT FOR EXPERIMENT 9 (continued) B. Qualitative Examination of Residue 1. Record what you observed when silver nitrate was added to the following: (a) Potassium chloride solution (b) Potassium chlorate solution (c) Residue solution 2. (a) What evidence did you observe that would lead you to believe that the residue was potassium chloride? (b) What would happen if you added silver nitrate to a solution of sodium chloride? Explain your answer. e) Did...
thermometer coffee cups containing reaction mixture When a 7.89-9 sample of solid potassium chlorate dissolves in...
thermometer coffee cups containing reaction mixture When a 7.89-9 sample of solid potassium chlorate dissolves in 32.0 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 20.00 °C to 3.899 °C. Calculate AH in kl/mol KCIOy for the solution process. KCIO,(s) - K*(aq) + CIO,'(aq) The specific heat of water is 4.18 3/ok Aucution - Kl/mol KCO,
Gummy bears decompose rapidly and explosively in molten potassium chlorate. Both decomposition and combustion react...
Gummy bears decompose rapidly and explosively in molten potassium chlorate. Both decomposition and combustion reactions happen simultaneously according to the balanced equation: C12H22011(s) + 8 KClO3(1) --> 12 CO2(g) + 11 H2O(g) + 8 KCl(aq) Using the AHºf values below, calculate the standard enthalpy change for this reaction. (Report your answer in standard notation.) C12H22011 (8) KCIO3 (1) CO2 (g) H2O (g) KCl (aq) A Hºf (kJ/mol) -2225.5 -397.73 -393.51 -241.82 -436.7 AH° rxn = * kJ
Percentage of Oxygen in Potassium Chlorate Introduction: The thermal decomposition of potassium chlorate can be described by the following equation: 2 KCIO3(s) 2 KCls) + 3 O2(g) Egn 1 (D stands for heating, elevated temperature) In this experiment you will determine the percentage of oxygen in potassium chlorate. You will compare the experimental result with the theoretical percentage calculated from the formula KCIO3. While potassium chlorate decomposes simply by heating, the reaction is very slow. A catalyst is used. Catalyst...
composition of potassium chlorate questions and problems
REPORT FOR EXPERIMENT 9 (continued) B. Qualitative Examination of Residue 1. Record what you observed when silver nitrate was added to the following: (a) Potassium chloride solution (b) Potassium chlorate solution (c) Residue solution 2. (a) What evidence did you observe that would lead you to believe that the residue was potassium chloride? (b) What would happen if you added silver nitrate to a solution of sodium chloride? Explain your answer. e) Did...
thermometer coffee cups containing reaction mixture When a 7.89-9 sample of solid potassium chlorate dissolves in 32.0 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 20.00 °C to 3.899 °C. Calculate AH in kl/mol KCIOy for the solution process. KCIO,(s) - K*(aq) + CIO,'(aq) The specific heat of water is 4.18 3/ok Aucution - Kl/mol KCO,
Gummy bears decompose rapidly and explosively in molten potassium chlorate. Both decomposition and combustion reactions happen simultaneously according to the balanced equation: C12H22011(s) + 8 KClO3(1) --> 12 CO2(g) + 11 H2O(g) + 8 KCl(aq) Using the AHºf values below, calculate the standard enthalpy change for this reaction. (Report your answer in standard notation.) C12H22011 (8) KCIO3 (1) CO2 (g) H2O (g) KCl (aq) A Hºf (kJ/mol) -2225.5 -397.73 -393.51 -241.82 -436.7 AH° rxn = * kJ
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