Be sure to answer all parts.Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions ofdollars every day. Although the actual process also requires water, a simplified equation (with rustshown as Fe,O is:4 Feb)+30,-2 Fe,0y)AH--165x 1e(a) What is the AH,. when 0.250 kg of iron rusts?x 10(b) How much rust forms when 3.90 x 10 kJ of heat is released?x 10g Fe,0< Prex1516Nexthp

a)The change in reaction enthalpy when 0.250 kg of iron rusts formed is calculated as follows,

Answered: Be sure to answer all parts.…

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter21: The Chemistry Of The Main Group Elements

Section: Chapter Questions

Problem 53PS

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In the presence of nitric acid, UO2+ undergoes a redox process. It is converted to UO22+ and nitric oxide (NO) gas is produced according to the following unbalanced equation: H+(aq)+NO3(aq)+UO2+(aq)NO(g)+UO22+(aq)+H2O(l) If 2.55 102 mL NO(g) is isolated at 29C and 1.5 atm, what amount (moles) of UO2+ was used in the reaction? (Hint: Balance the reaction by the oxidation states method.)
(a) When the metallic element sodium combines with thenonmetallic element bromine, Br2(l), what is the chemicalformula of the product? (b) Is the product a solid, liquid, orgas at room temperature? (c) In the balanced chemical equationfor this reaction, what is the coefficient in front of theproduct if the coefficient in front of Br2(l) is 1?
A typical formulation for window glass is 75% SiO₂, 15% Na₂O, and 10.% CaO by mass. What masses of sand (SiO₂),sodium carbonate, and calcium carbonate must be combined toproduce 1.00 kg of glass after carbon dioxide is driven off bythermal decomposition of the carbonates?
Aircraft de-icing agents, such as propylene glycol [1,2-propanediol; CH₃CH(OH)CH₂OH; d=1.036 g/mL], are used toremove ice and snow prior to winter flights, but their presence inrunoff depletes O₂ in natural waters. (a) Write a balanced equa-tion for the complete oxidation of propylene glycol by O₂.(b) What is the “theoretical oxygen demand,” in grams of O₂ required per gram of propylene glycol oxidized? (c) What is thetheoretical oxygen demand, in grams of O₂ required per liter ofsolution, of 90.0% by volume aqueous propylene glycol?
What coefficients balance the following chemical equation? ___C2H2 + ___O2 ---> ___CO2 + ___H2O
The compound diborane (B2H6) was at one time considered for use as a rocket fuel. Its combustion reaction is B2H6(g) + 3 O2(l) → 2 HBO2(g) + 2 H2O(l) The fact that HBO2, a reactive compound, was produced rather than the relatively inert B2O3 was a factor in the discontinuation of the investigation of the diborane as a fuel. What mass of liquid oxygen (LOX) would be needed to burn 234.4 g of B2H6? Answer in units of g.
The compound diborane (B2H6) was at one time considered for use as a rocket fuel. Its combustion reaction is B2H6(g) + 3 O2(l) → 2 HBO2(g) + 2 H2O(l). The fact that HBO2, a reactive compound, was produced rather than the relatively inert B2O3 was a factor in the discontinuation of the investigation of the diborane as a fuel. What mass of liquid oxygen (LOX) would be needed to burn 234.4 g of B2H6? Answer in units of g. (part 2 of 2) What mass of HBO2 is produced from the combustion of 94.7 g of B2H6? Answer in units of g.
A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas city (MCI) to Baltimore (BWI) burned 11800 lb. of Jet A fuel. Jet A fuel is kerosene based, consisting primarily of CnH2n+2 hydrocarbons, with n = 6 to 16, so the Carbon:Hydrogen ratio is close to 1:2. During this flight , how much CO2 (in kg) was released into the atmosphere? (assume the combustion of fuel was complete, so all fuel was converted into H2O and CO2).
An Olympic gold medal must contain a minimum of 6 grams of gold (MW = 196.97 g/mol) and has at least 92.5% silver. Supposedly, each medal is made by coating a 60-mm diameter, 3-mm thick, gold-free silver alloy disk with gold via electrolytic deposition using a gold (III) solution, what is the time required in hours to finish plating all the gold medals used in the Tokyo Olympics with minimum gold content if the available electricity source can deliver 50 amperes of current?
If 6.43 A is applied for 79 minutes, what mass of Cr(s) will be produced? ____ g Cr
Magnesium nitrate and barium nitrate decompose similarly on heating and the reaction can be represented as follow: M(NO3)2 (s) --› MO (s) + 2NO2 (g) + ½O2 (g), where M = Mg or Ba (a) When Group 1 nitrates (with the exception of lithium nitrate) are strongly heated, the corresponding nitrite was formed along with a colorless gas which relights a glowing splint. (i) Write a balanced equation for the thermal decomposition of potassium nitrate. (ii) Unlike other Group 1 nitrates, lithium nitrate decomposes on heating in the same way as Group 2 nitrates. Suggest a reason for the difference in behaviour, and give an equation for its decomposition. (b) Zinc carbonate and magnesium carbonate decompose when heated to give similar products. (i) Suggest an equation for the thermal decomposition of magnesium carbonate. (ii) The radius of Zn2+ cation is 0.074 nm. Use the Data Booklet to deduce whether zinc carbonate will decompose at a higher or lower temperature than magnesium carbonate. Explain…
Titanium is a strong, slightly corrosion resistant metal and is used in rockets, airplanes, jet engines and bicycle frame structures. It is obtained from the reaction of titanium (IV) and molten magnesium between 950 C and 1150 ºC. TiCl4 (g) + Mg (s) → Ti (s) + MgCl2 (s) In a certain industrial process, when 3,54x107 g TiCl4 and 1,13x107 g Mg react, 7,91x106 g Ti is obtained; a) limiting component b) theoretical yield c) actual yield d) Calculate the percentage yield.

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