Titanium oxide (TiO2) is reduced by carbon to form titanium metal and carbon monoxide (CO). If 5.00g of TiO2 is reacted with 10.0 g of C, which reactant is the limiting reagent?
Titanium oxide (TiO2) is reduced by carbon to form titanium metal and carbon monoxide (CO). If...
Experiment 9-Post-lab Questions 1. Methanol (CH,OH) can be produced by the reaction of carbon monoxide (CO) with hydrogen (H,). The balanced chemical reaction is: cO@)+2 H, (g)CH,OH() Suppose 14.0 g of carbon monoxide is reacted with 8.0 g of hydrogen. a. Which reactant is the limiting reagent? b. What is the theoretical yield for methanol? c. At the completion of the reaction, how many grams of the excess reagent will remain? 2. Iron(III) oxide (Fe,O,) can be converted to iron...
Titanium(IV) oxide is converted to titanium carbide with carbon at a high temperature. Calculate ΔrG° and K at 891°C. Titanium(IV) oxide is converted to titanium carbide with carbon at a high temperature. TiO2 (s) + 3 C(s) + 2 CO(g) + TiC(s) Compound AfGº (kJ/mol) TiO2 (s) -728.24 TiC(s) -159.09 CO(g) -214.92 a Calculate A,Gº and K at 891 °C. AG = kJ K=
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.
Consider the reaction between solid iron(III) oxide and carbon monoxide gas to form carbon dioxide gas and solid iron (11,111) oxide. If carbon monoxide is present in excess, determine the amount of iron(III) oxide needed to produce 2.21x1024 iron (11,HI) oxide molecules. O 1.83 moles 3.67 moles 07.34 moles O 11.0 moles O 5.50 moles 0.50 mol A, 0.60 mol B, and 0.90 mol C are reacted according to the following reaction A + 2B + 3C 2D + E...
Can somebody help me solve this?? Titanium (IV) oxide is converted to titanium carbide with carbon at high temperature. TiO2(s) + 3 C(s) --> 2 CO(g) + TiC(s) compound free energies of formation at 727°C, kJ/mol TiO2(s) -757.8 TiC(s) - 162.6 -200.2 CO(g) Calculate K
Nickel (II) oxide reacts with carbon monoxide to form nickel metal. CO(g) + NiO(s) ⇄ CO2(g) + Ni(s) Kp = 20 at 873 K If a reaction vessel at equilibrium contains solid Ni, solid NiO, 400 mm Hg of CO2, and 20 mm Hg of CO, doubling the amount of CO(g) present will lead to the production of more solid nickel at 873 K. A) True B) False
5. The first step in the commercial production of titanium metal is the reaction of TiO2 with chlorine an graphite: TiO2 (s) + 2 Clz (g) + 2 C(s) TiCl4 (1) + 2 CO (g) Calculate AGⓇ for the reaction. Substance AG? (kJ/mol Substance AG® (kJ/mol) C() 0 TiCl4 (1) -804.2 CO(g) -110.5 TiO2 (s) -944.0 121.3 Cl2 (g)
5. The first step in the commercial production of titanium metal is the reaction of TiO2 with chlorine and graphite: TiO2 (s) + 2 Cl2 (g) + 2 C(s) TiCl4 (1) + 2 CO (g) Calculate AGº for the reaction. Substance AG? (kJ/mol) Substance AG (kJ/mol) C(s) 0 TiCl4 (1) -804.2 CO (g) -110.5 TiO2 (s) -944.0 Cl2 (8) 121.3
Name TA Laboratory Date - Section Experiment 9-Post-lab Questions 1. Methanol (CH,OH) can be produced by the reaction of carbon monoxide (CO) with hydrogen (H). The balanced chemical reaction is: CÓg) + 2 H (8) -CH,OH() Suppose 14.0 g of carbon monoxide is reacted with 8.0 g of hydrogen. a. Which reactant is the limiting reagent? b. What is the theoretical yield for methanol? c. At the completion of the reaction, how many grams of the excess reagent will remain?...
are these right? im having a hard time on number 2 a-c Experiment 9-Post-lab Questions 1. Methanol (CH,OH) can be produced by the reaction o balanced chemical reaction is by the reaction of carbon monoxide (CO) with hydrogen (H). The CO(g) + 2 H (g)-CH2OH) Suppose 14.0 g of carbon monoxide is reacted with 8.0 g of hydrogen 3. Which reactant is the limiting reagent? Carbon monoxide (co) b. What is the theoretical yield for methanol? 16.02 g CH₂OH c....