(a)
Interpretation:
The balanced chemical equation for the reaction of sodium sulfite and hydrochloric acid should be written.
Concept introduction:
A balanced chemical equation is defined as reaction in which there are same number of constituent atoms on both side of the reaction arrow, that is reactant and product side.
(a)
Answer to Problem 12.110PAE
Solution: Balanced chemical equation.
Explanation of Solution
Here, sulfur dioxide, sodium chloride and water are formed when sodium hydrogen sulfite is reacted with hydrochloric acid. The balanced reaction is as follows:
(b)
Interpretation: Mass of
Concept introduction:
For a reaction, if any reactant is present in excess, the mass of product obtained depends on the limiting reactant. The ratio of number of moles remains the same for any reaction.
Number of mole is related to mass and molar mass as follows:
where, n is the number of moles
m is mass
M is molar mass
(b)
Answer to Problem 12.110PAE
Solution: Amount of sulfur dioxide produced is
Explanation of Solution
The balanced
Here, HCl is present in excess, thus,
Calculate the number of moles of
Molecular mass of
Thus,
Since,
Now, calculate mass of
Molar mass of
Thus,
Therefore, 1.2 g of SO2 is produced from 1.9 g of
(c)
Interpretation: Equilibrium concentration of each species in the given reaction should be identified.
Concept introduction: For a general reaction,
Expression for the equilibrium constant (K) is as follows:
Also, concentration or molarity of a solution is defined as number of moles in 1 L of solution. The unit of concentration or molarity is mol/L or M.
(c)
Answer to Problem 12.110PAE
Solution: Equilibrium concentration of
Equilibrium concentration of
Equilibrium concentration of
Explanation of Solution
Given reaction is
Equilibrium constant for the reaction will be:
The ICE table for the reaction will be:
Initial | |||
Change | |||
equilibrium |
Since, the value of equilibrium constant is very high thus, SO2 completely react with oxygen to form SO3. The number of moles of SO2 remain will be zero.
Thus,
Calculate number of moles of O2 remain as follows:
Moles of O2 remain,
And,
Concentration can be calculated as follows:
Since, volume of container is 100 mL or 0.1 L, equilibrium concentration of all species can be calculated.
Therefore, equilibrium concentration of SO2, O2 and SO3 is 0 M, 0.41 M and 0.183 M respectively.
Want to see more full solutions like this?
Chapter 12 Solutions
Chemistry for Engineering Students
- (a) Write chemical equations to show what happens when each of the following substances is mixedwith water:(i) Hydride ion(ii) Glucose, C6H12O6(s)(iii) Copper(II) bromide(iv) Formic acid(b) Write chemical equations for the following processes:(i) Chemical reaction for ΔH°f for mercury(I) phosphate.(ii) Thermal dissociation of gaseous bromine.(iii) Sublimation of carbon dioxide.(iv) Reduction of VO2+ to produce VO2+.(v) Neutralization of sulfuric acid by barium hydroxide.(vi) Thermal decomposition of 1 mol of sodium bicarbonate to produce sodium carbonate, carbon dioxide and waterarrow_forwardWrite the balanced chemical equation for conversion of Al(s) to KAl(SO4)2·12H2O(s) in aqueous solution.arrow_forwardSuppose Cao is placed in a vacuum in which the partial pressure of oxygen is 10-r mm Hg. Will Cao be reduced?arrow_forward
- The value of Ka for nitrous acid 1HNO22 at 25 °C is given in Appendix D. (a) Write the chemical equation for the equilibrium that corresponds to Ka.arrow_forwardWrite an expression for the equilibrium constant for this reaction: N2O4(g)+ O3(g)=N2O5(s)+O2(g)arrow_forwardCalculate the equilibrium partial pressure of NO2 and N2O4.arrow_forward
- The equilibrium constant for the reaction, 3 H2(g) + N2(g)= 2NH3(g), at a given temperature is 1.4 x 10–7. Calculate the equilibrium concentration of ammonia, if [H2] = 1.2 x 10–2 mol L–1 and [N2] = 3.2 x 10–3 mol L–1.arrow_forwardWhat pressure is required to achieve a CO2 concentration of 0.0690 mol L-l at 20°C?arrow_forwardBoron nitride (BN) has a structure similar to graphite, but is a white insulator rather than a black conductor. It is synthesized by heating diboron trioxide with ammonia at about 1000°C. (a) Write a balanced equation for the formation of BN; water forms also.(b) Calculate ΔH°rxn for the production of BN (ΔH°f of BN is -254 kJ/mol).(c) Boron is obtained from the mineral borax, Na₂B₄O₇.10H₂O.How much borax is needed to produce 1.0 kg of BN, assuming 72% yield?arrow_forward
- Take about 5 ml of dil. HCl in a test tube and add a few pieces of fine granules to it.Which gas is evolved?(a) Chlorine(b) Hydrogen(c) HCl(d) Nitrogenarrow_forwardBoric acid, H3BO3, is not a Brønsted-Lowry acid but a Lewis acid.(a) Write an equation for its reaction with water.(b) Predict the shape of the anion thus formed.(c) What is the hybridization on the boron consistent with the shape you have predicted?arrow_forwardTetraphosphorus decaoxide (P₄O₁₀) is made from phos-phate rock and used as a drying agent in the laboratory.(a) Write a balanced equation for its reaction with water.(b) What is the pH of a solution formed from the addition of 8.5 g of P₄O₁₀ in sufficient water to form 0.750 L?arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning