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Based on the positions in the periodic table, which of the following reactions would you expect to occur?
(a)
(c)
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Chapter 4 Solutions
Chemistry, Books a la Carte Plus Mastering Chemistry with eText -- Access Card Package (7th Edition)
- The reduction of iron(III) oxide to iron during steel-making can be summarized by this sequence of reactions: 2C (s) + O, (g) =2 CO (g) K1 Fe,0, (s)+ 3 CO (g) =2 Fe (1)+ 3 CO, (g) K2 The net reaction is: 2 Fe,0, (s)+ 6 C (s)+ 3 O, (g) – 4 Fe (1)+ 6 CO, (g) K Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K, and K,. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. Karrow_forwardTitanium occurs in the magnetic mineral ilmenite (FeTiO3), which is often found mixed up with sand. The ilmenite can be separated from the sand with magnets. The titanium can then be extracted from the ilmenite by the following set of reactions: FeTiO3(s)+3Cl₂ (g)+3C(s)→3CO(g)+FeCl₂ (s)+TiCl (9) TiCl4 (g)+2Mg(s)→2MgCl₂ (1)+Ti(s) Suppose that an ilmenite-sand mixture contains 24.6 % ilmenite by mass and that the first reaction is carried out with a 90.6% yield. Part A If the second reaction is carried out with an 86.3 % yield, what mass of titanium can be obtained from 1.10 kg of the ilmenite-sand mixture? Express your answer with the appropriate units. mTi = Submit O μÀ Value Request Answer Units www Review | Constants | Perio ?arrow_forwardproceed as W KNUD TE 6. Does the chemical reaction represented by 2Au(s) + 2HNO3(aq) →→→ 2AuNO3(aq) + H₂(g) proceed as written? Gold is a relatively useful metal for certain applications, such as jewelry and electronics. Does your answer suggest why this is so?arrow_forward
- The reduction of iron(III) oxide to iron during steel-making can be summarized by this sequence of reactions: 20(s) +0, (g) =2 CO (g) K, Fe,0, (s) +3 CO (g) =2 Fe (1) +3 CO, (g) K2 The net reaction is: 2 Fe,O, (s) +6C (s) +30, (g)=4 Fe (1) +6CO, (3) K Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K, and K,. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K = 믐 Submit Assign Continue MacBook Air F7 000 吕口 000 FA F5arrow_forward2- C₂²- 1 + 2 (s) Complete and balance the following redox reaction in basic solution. Be sure to include the proper phases for all species within the reaction. 103(aq) + Re(s) → ReO4 (aq) +10¯(aq) 3 ( I Reset 4 Question 14 of 28 (1) LO 5 OH ) 6 O 7 (g) 个 1 8 9 (aq) Re 0 Xarrow_forwardBalance the following reaction by filling in the blank with a single product. Treat subscripts and superscripts as regular numbers. A3B3C* → A2C +arrow_forward
- When potassium metal is placed in water, a large amount of energy is released as potassium hydroxide and hydrogen gas are produced in the reaction 2K(s) + 2H2O(l) → 2KOH(aq) + H2(g). Your lab partner says this is a redox reaction and a combustion reaction. Do you agree? Defend your answer by explaining whether or not it meets the requirements of each type of reaction.arrow_forwardThe reaction between nitrogen and oxygen is given below: Nz() + O2(g) → 2 NO(g) We therefore know that which of the following reactions can also occur? O2 NO,() + 2 NO(2) + Oz(g) ON,0(g) +2 NH3(g) +2 02(g) O2 NO(2) + O2(g)→ 2 NO:(g) O None of the Above Submit Answer Try Another Version 6 item attempts remainingarrow_forwardThere are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(I) oxide and sulfur dioxide: 2 Cu, S(s)+3 O,(g)→2 Cu,O(s)+2 SO,(g) In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: Cu,O(s)+C(s)→2 Cu(s)+CO(g) Write the net chemical equation for the production of copper from copper(I) sulfide, oxygen and carbon. Be sure your equation is balanced. O-0arrow_forward
- 2 SmCl3(aq) + 6 LiCl(aq) + 6 e- → 2 Sm(s) + 6 Li+(aq) + 6 Cl-(aq) how di you get this reaction , i provided a different onearrow_forwardSelenic acid, H2SeO4, is produced from elemental selenium in a two-stage reaction. First the selenium isoxidized to selenous acid by nitric acid. Then the selenous acid is oxidized by potassium permanganate toselenic acid. The equations are:3 Se (s) + 4 HNO3 (l) + H2O (l) → 3 H2SeO3 (aq) + 4 NO (g)8 H2SeO3 (aq) + 2 KMnO4 (aq) → 5 H2SeO4 (aq)+ K2SeO3 (aq)+ 2 MnSeO3 (aq) + 3 H2O (l)What mass of selenic acid (in kg) can be produced from 1.00 kg of Se?Molar masses (g/mol): Se 78.96 H2SeO4 144.97arrow_forwardPart 1 A student carried out an investigation to observe the effect of changing concentration of sulfuric acid on the breakdown of calcium carbonate (marble) chips. They changed the concentration of the acid between each test but kept the size of the marble chips constant. The full equation for the reaction and a graph of the overall results can be seen below. CaCO3(s) + H₂SO4(aq) → CaSO4(aq) + CO2(g) + H₂O (1) a) b) Rate of Reaction * Concentration of Acid (mol dm³) Explain, using collision theory, why the student obtained these results, and state what they could conclude about the effect of changing concentration of acid on the rate of reaction between calcium carbonate and sulfuric acid. If the student had ground up the calcium carbonate chips into a powder and run the tests again, what would you expect to happen to the rate of reaction? Briefly explain why by applying collision theory. Part 2 The student ran the same experiment, but this time changed the temperature, increasing it…arrow_forward
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