Homework Answers
To balance a chemical equation count the number of atoms of each element on both sides of the reaction and equalise them by adding suitable coefficients.
Balanced equation for this reaction is,
Fe2O3 + 2Al --------> Al2O3 + 2Fe
Answer = a. 1 , 2 , 1 , 2
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the coefficienfs are respectively _______ for the following
equation.
Fe2O3+Al --> Al2O3+Fe
The coefficients are respectively...
help !! QUESTION 8 Consider the reaction: Fe2O3 + 2AI 2Fe + Al2O3 In this reaction,...
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QUESTION 8 Consider the reaction: Fe2O3 + 2AI 2Fe + Al2O3 In this reaction, which substances are the reducing agent and oxidizing agent, respectively? a. Al and Fe2O3 b. Fe2O3 and Al OC. Al and A1203 Od. Fe and Fe203 e none of these choices is correct
1. when the chemical equation Fe2O3(s)+C(s) (arrow) Fe(s) +CO(g) is balanced, the coefficients in order will...
1. when the chemical equation Fe2O3(s)+C(s) (arrow) Fe(s) +CO(g) is balanced, the coefficients in order will be: 2. In a chemical reaction, the symbol "(s)" may be read as: a)solution b) solid c) soluble d) state 3. A reactant in the chemical reaction Cl2 (g) + 2NABr (aq) arrow 2NACl(aq) + Br2(aq) is: a) chlorine b) sodium chloride c) bromine d) none of the above 4. The reaction Al2O3(s) +6HCl(aq) arrow 2AlCl3(aq) +3H2O(I) is a balanced equation. 5. What is...
3) Answer all parts of the following question. a. The reaction: Al(s) + Fe2O3(s) → Fe(s)...
3) Answer all parts of the following question. a. The reaction: Al(s) + Fe2O3(s) → Fe(s) + Al2O3(s) has ΔH = -847.6 kJ and ΔS = -41.3 J/K at 25°C. Calculate ΔG and determine if it is spontaneous. b. Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) ΔH = -11.0 kJ; ΔS = -17.4 J/K c. Find ΔSsurr and predict whether or not this reaction will be spontaneous at 398 K. NH3(g)...
correct Question 4 0/2 pts Fe2O3(s) + 2Al(s) Al2O3(s) + 2 Fe(s) AH° = -851.5 kJ/mol...
correct Question 4 0/2 pts Fe2O3(s) + 2Al(s) Al2O3(s) + 2 Fe(s) AH° = -851.5 kJ/mol If 75 g Fe2O3 is combined with 23 g Al, what is the value of q (kJ)? Enter your answer as an integer. 726
How much energy is evolved during the formation of 197 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s)...
How much energy is evolved during the formation of 197 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJ A. 964 kJ B. 1.52 x 103 kJ C. 3.02 x 103 kJ D. 482 kJ E. 8.40 x 103 kJ
10.Calculate the standard enthalpy change for the reaction 2Al(s) + Fe2O3(s) →2Fe(s) + Al2O3(s) given that...
Calculate the standard enthalpy change for the reaction 2Al(s)+Fe2O3(s) → 2Fe(s)+Al2O3(s)given that2 Al(s)+ 3/2O2(g) → Al2O3(s) ΔHrxn°=-1669.8 kJ/mol2 Fe(s)+3/2O2(g) → Fe2O3(s) ΔHrxn°=-822.2 kJ / mol
Aluminum oxide (Al2O3) is produced according to the following equation. 4 Al(s) + 3 O2(g) →...
Aluminum oxide (Al2O3) is produced according to the following equation. 4 Al(s) + 3 O2(g) → 2 Al2O3(s) If the reaction occurs with an 82.4% yield, what mass of aluminum should be reacted with excess oxygen to produce 45.0 grams of Al2O3? a. 54.6 g Al b. 37.9 g Al c. 35.1 g Al d. 23.8 g Al e. 28.9 g Al How do we solve this problem
4 Consider the balanced chemical equation: 2Al(s) + Fe2O3(s) — 2Fe(s) + Al2O3(s) heat of reaction...
4 Consider the balanced chemical equation: 2Al(s) + Fe2O3(s) — 2Fe(s) + Al2O3(s) heat of reaction = -851.5 kJ (a) How many kilojoules of heat are produced when 4.88 moles of Al react? (b) How many kilojoules of heat are produced when 4.88 moles of Fe2O3 react? (c) What mass of Fe2O3 must react to produce 387 kJ of heat?
3.(15pts) In each case, find the missing AH. (kJ/mole) (a) If 2 Al(s) + Fe2O3(s) ---->...
3.(15pts) In each case, find the missing AH. (kJ/mole) (a) If 2 Al(s) + Fe2O3(s) ----> Al2O3(s) + 2 Fe(s) AH,xº = -851.5kJ/mol then 1/8 Al2O3(s) + 1/4 Fe(s) --> 1/4 Al(s) + 1/8 Fe2O3(s) AHX = ? (b) If CaO(8) + 3 C(s) --> CaC2(s) + CO(g) AH,” = 464,8 kJ/mol then 6 CaO(s) + 18 C(s) ---> 6 CaCz(s) +6 CO(g) AHX = ? (c) If N2(g) + 2 O2(g) ---> N204(g) and 2 NO2(g) ----> N2(g) +...
2. When the following equation is balanced with the smallest possible integer coefficients, what is the...
2. When the following equation is balanced with the smallest possible integer coefficients, what is the coefficient of H'? _Cr* __H __ Cr +_ He A) 3 B) 5 C6 D)2 E) 4 3. The following reaction occurs in acidic aqueous solution: H.AsO + Zn = AsH, + Zn? H.ASO. is a[n) agent in which the oxidation number of Asis C ) reducing. 13 A) reducing 5 D) oxidizing, +3 B) oxidizing, + 5 E) reducing. +2 When the following...
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QUESTION 8 Consider the reaction: Fe2O3 + 2AI 2Fe + Al2O3 In this reaction, which substances are the reducing agent and oxidizing agent, respectively? a. Al and Fe2O3 b. Fe2O3 and Al OC. Al and A1203 Od. Fe and Fe203 e none of these choices is correct
correct Question 4 0/2 pts Fe2O3(s) + 2Al(s) Al2O3(s) + 2 Fe(s) AH° = -851.5 kJ/mol If 75 g Fe2O3 is combined with 23 g Al, what is the value of q (kJ)? Enter your answer as an integer. 726
4 Consider the balanced chemical equation: 2Al(s) + Fe2O3(s) — 2Fe(s) + Al2O3(s) heat of reaction = -851.5 kJ (a) How many kilojoules of heat are produced when 4.88 moles of Al react? (b) How many kilojoules of heat are produced when 4.88 moles of Fe2O3 react? (c) What mass of Fe2O3 must react to produce 387 kJ of heat?
3.(15pts) In each case, find the missing AH. (kJ/mole) (a) If 2 Al(s) + Fe2O3(s) ----> Al2O3(s) + 2 Fe(s) AH,xº = -851.5kJ/mol then 1/8 Al2O3(s) + 1/4 Fe(s) --> 1/4 Al(s) + 1/8 Fe2O3(s) AHX = ? (b) If CaO(8) + 3 C(s) --> CaC2(s) + CO(g) AH,” = 464,8 kJ/mol then 6 CaO(s) + 18 C(s) ---> 6 CaCz(s) +6 CO(g) AHX = ? (c) If N2(g) + 2 O2(g) ---> N204(g) and 2 NO2(g) ----> N2(g) +...
2. When the following equation is balanced with the smallest possible integer coefficients, what is the coefficient of H'? _Cr* __H __ Cr +_ He A) 3 B) 5 C6 D)2 E) 4 3. The following reaction occurs in acidic aqueous solution: H.AsO + Zn = AsH, + Zn? H.ASO. is a[n) agent in which the oxidation number of Asis C ) reducing. 13 A) reducing 5 D) oxidizing, +3 B) oxidizing, + 5 E) reducing. +2 When the following...
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