The mass percent of titanium dioxide (TiO2) in an ore can be evaluated by carrying out...
The mass percent of titanium dioxide (TiO2) in an ore can be evaluated by carrying out the following reaction and measure the amount of O2 gas produced.
3TiO2 (s) + 4BrF3 (l) = 3TiF4 (s) + 2Br2 (l) + 3O2 (g)
If 2.376 of a TiO2-containing ore generates 0.143g of O2, what is the mass percent of TiO2 in the ore sample?
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The mass percent of titanium dioxide (TiO2) in an ore
can be evaluated by carrying out...
QUESTION 5 The combustion of titanium with oxygen produces titanium dioxide: Ti(s) + O2(g) → TiO2(s)...
QUESTION 5 The combustion of titanium with oxygen produces titanium dioxide: Ti(s) + O2(g) → TiO2(s) When 2.060 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 91.60 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimeter is kulmol 19.6 -1.52 × 104 -0.154 O-311 14.3 QUESTION...
1. Titanium dioxide particles are used to brighten paints. They are produced by gas-phase oxidation of...
1. Titanium dioxide particles are used to brighten paints. They are produced by gas-phase oxidation of TiCl4 vapor in a hydrocarbon flame. The dominant reaction is hydrolysis, TICI4 + 2H20 à TiO2(s) + 4HCI The reaction rate is first-order in TiCl4 and zero-order in H20. The rate constant for the reaction is: k=8X104exp-88000 J/molRgT S-1 The reaction takes place at 1200 K in a constant pressure flow reactor at 1 atm pressure (1.01 X 105 Pa). The gas composition at...
Titanium reacts with bromine gas according to the following balanced chemical equation: 2Ti(s)+3Br2(l)→2TiBr3(s) A: What mass...
Titanium reacts with bromine gas according to the following balanced chemical equation: 2Ti(s)+3Br2(l)→2TiBr3(s) A: What mass of titanium(III) bromide is produced when 139.29 g titanium reacts with 553.73 g bromine liquid? in gTiBr3 B: What is the percent yield of titanium(III) bromide if 556.03 g of titanium(III) bromide is actually obtained?
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.
1.Sodium hydrogen carbonate, NaHCO3, can be decomposed completely by heating. 2 NaHCO3(s) → Na2CO3(s) + CO2(g)...
1.Sodium hydrogen carbonate, NaHCO3, can be decomposed completely by heating. 2 NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g) A sample of impure NaHCO3 with an initial mass of 0.739 g yielded a solid residue (consisting of Na2CO3 and other solids) with a final mass of 0.564 g. Determine the mass percent of NaHCO3 in the sample. 2.In a process for producing acetic acid, oxygen gas is bubbled into acetaldehyde, CH3CHO, containing manganese(II) acetate (catalyst) under pressure at 60°C. 2CH3CHO(l) +...
1. Moles of Reactant to Mass of Reactant: Identify the iodide ions and ozone in the...
1. Moles of Reactant to Mass of Reactant: Identify the iodide ions and ozone in the balanced chemical equation. Use mole ratio, then convert to grams. A method used by the EPA for determining the ozone concentration in the air is to pass an air sample through a bubbler containing iodide ions. The iodide ions remove the ozone according to the following reaction: O3(g) + 2 I-(aq) + H2O(l) → O2(g) + I2(aq) + 2 OH-(aq) How many grams of ozone...
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid,...
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO,(s) + 4 HCl(aq) + MnCl2(aq) + 2 H,0(1) + Cl2(g) How much Mno,(s) should be added to excess HCl(aq) to obtain 275 mL CI,(e) at 25°C and 725 Torr? mass of Mno, Solid ammonium chloride, NH,CI, is formed by the reaction of gaseous ammonia, NH,, and hydrogen chloride, HCI. NH,() + HCI(g) →NH,Cl(s) A 4.70 g...
2. What is the percent yield or if the reaction of 25.0 g P. and 1596....
2. What is the percent yield or if the reaction of 25.0 g P. and 1596. produces 104 g PCI? P.(s) + Cl2(o) PCA) If the reaction produces 5.3 mg of carbon dioxide how many grams of water are produced? d. How many grams of oxygen are needed to react with 6.00 x 10molecules of CH? 3. How many grams of aluminum chloride are formed when 30.0 grams of aluminum are reacted with gas? a. Write the balance equation b....
please help me calculate. Note: The mass of carbon dioxide gas produced during the reaction can...
please help me calculate.
Note: The mass of carbon dioxide gas produced during the reaction can be determined by how m mass was lost from the chemical reaction. Think about it for a moment; those bubbles that were forming carbon dioxide gas molecules escaping from the beaker, while all the other chemicals remained behind. You must first compute the combined mass of vinegar and baking soda you started with, and from this subtract the mass of your solution after the...
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid,...
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation Mno,(s) + 4 HCl(aq) — MnCI, (aq) + 2 H2O(l) + Cl2(g) How much MnO,(s) should be added to excess HCl(aq) to obtain 125 mL CI(g)at 25 °C and 805 Torr? mass of MnO,: A 4.05 g sample of an unknown gas at 29 °C and 1,00 atm is stored in a 2.35 L flask. What is...
QUESTION 5 The combustion of titanium with oxygen produces titanium dioxide: Ti(s) + O2(g) → TiO2(s) When 2.060 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 91.60 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimeter is kulmol 19.6 -1.52 × 104 -0.154 O-311 14.3 QUESTION...
1. Titanium dioxide particles are used to brighten paints. They are produced by gas-phase oxidation of TiCl4 vapor in a hydrocarbon flame. The dominant reaction is hydrolysis, TICI4 + 2H20 à TiO2(s) + 4HCI The reaction rate is first-order in TiCl4 and zero-order in H20. The rate constant for the reaction is: k=8X104exp-88000 J/molRgT S-1 The reaction takes place at 1200 K in a constant pressure flow reactor at 1 atm pressure (1.01 X 105 Pa). The gas composition at...
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.
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO,(s) + 4 HCl(aq) + MnCl2(aq) + 2 H,0(1) + Cl2(g) How much Mno,(s) should be added to excess HCl(aq) to obtain 275 mL CI,(e) at 25°C and 725 Torr? mass of Mno, Solid ammonium chloride, NH,CI, is formed by the reaction of gaseous ammonia, NH,, and hydrogen chloride, HCI. NH,() + HCI(g) →NH,Cl(s) A 4.70 g...
2. What is the percent yield or if the reaction of 25.0 g P. and 1596. produces 104 g PCI? P.(s) + Cl2(o) PCA) If the reaction produces 5.3 mg of carbon dioxide how many grams of water are produced? d. How many grams of oxygen are needed to react with 6.00 x 10molecules of CH? 3. How many grams of aluminum chloride are formed when 30.0 grams of aluminum are reacted with gas? a. Write the balance equation b....
please help me calculate.
Note: The mass of carbon dioxide gas produced during the reaction can be determined by how m mass was lost from the chemical reaction. Think about it for a moment; those bubbles that were forming carbon dioxide gas molecules escaping from the beaker, while all the other chemicals remained behind. You must first compute the combined mass of vinegar and baking soda you started with, and from this subtract the mass of your solution after the...
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation Mno,(s) + 4 HCl(aq) — MnCI, (aq) + 2 H2O(l) + Cl2(g) How much MnO,(s) should be added to excess HCl(aq) to obtain 125 mL CI(g)at 25 °C and 805 Torr? mass of MnO,: A 4.05 g sample of an unknown gas at 29 °C and 1,00 atm is stored in a 2.35 L flask. What is...
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