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Stoichiometry, Stoichiometric Calculations And Limiting Reagent - (Concept)
Stoichiometry:
Stoichiometry deals with the calculation of masses (sometimes volumes also) of the reactants and the products involved in a chemical reaction. Before understanding how to calculate the amounts of reactants required or the products produced in a chemical reaction, let us study what information is available from the balanced chemical equation of a given reaction.
Stoichiometric Calculations:
Step 1 Write down the correct formulas of reactants and products.
Step 2 Balance the number of atoms on both reactant and product sides.
Step 3 Make the equation balanced.
The coefficients of atoms or molecules are stoichiometric coefficients.
Limiting Reagent:
The reactant is consumed first in the reaction. When we are dealing with the balanced chemical equation, if the number of moles of reactants is not in the ratio of the stoichiometric coefficient of the balanced chemical equation, then there should be one reactant that should be limiting reactant.
% yield
Sometimes, experimentally, the reaction does not undergo 100% completion because of many factors which are involved in the actual industrial processes. So in such cases, we need the concept of % yield.
It is defined as the ratio of actual moles of product(s) formed to the number of moles that should have been theoretically formed assuming 100% completion of the reaction.
| Exam | Chapter |
| JEE MAIN | Some basic concepts in chemistry |
The minimum amount of consumed per gram of reactant is for the reaction :
(Given atomic mass :
,
)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
For a reaction,
In which of the following reaction mixtures, H2 is limiting reagent?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The ammonia released on the quantitative reaction of 0.6g, urea
with sodium hydroxide
can be neutralized by:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
$\mathrm{CaCO}_3 \xrightarrow{\Delta} \mathrm{CaO}+\mathrm{CO}_2$
Number of moles of CaCO3 needed to be heated to release 33.6 L of CO2 at STP ____ $\times$10−1
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The formula of a gaseous hydrocarbon which requires 6 times of its own volume of $\mathrm{O}_2$ for complete oxidation and produces 4 times its own volume of $\mathrm{CO}_2$ is $C_x H_y$. The value of y is __________.
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Complete combustion of 1.80g of an oxygen-containing compound $\left(C_x H_y O_z\right)$ gave 2.64 g of CO2 and 1.08 g of $\mathrm{H}_2 \mathrm{O}$. The percentage of oxygen in the organic compound is:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Complete combustion of 750 g of an organic compound provides 420 g of $\mathrm{CO}_2$ and 210 g of $\mathrm{H}_2 \mathrm{O}$. The percentage composition of carbon and hydrogen in organic compound is 15.3 and . _________ respectively. (Round off to the Nearest Integer)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
_________ grams of 3-Hydroxy propanal (MW=74) must be dehydrated to produce 7.8 g of acrolein (MW = 56) (C3H4O) if the percentage yield is 64. (Round off to the Nearest Integer).
[Given : Atomic masses : C : 12.0 u, H : 1.0 u, O : 16.0 u ]
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The mass of ammonia in grams produced when 2.8 kg of dinitrogen quantitatively reacts with 1 kg of dihydrogen is_________
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The minimum number of moles of O2 required for complete combustion of 1 mole of propane and 2 moles of butane is ______
| A. |
|
| B. |
|
| C. |
|
| D. |
|
If a rocket runs on fuel and liquid oxygen,the weight of oxygen required and
released for every litre of fuel respectively are:
(Given: density of the fuel is )
| A. |
|
| B. |
|
| C. |
|
| D. |
|
120 g of an organic compound that contains only carbon and hydrogen gives 330 g of , and 270 g of water on complete combustion, The percentage of carbon and hydrogen, respectively are
| A. |
|
| B. |
|
| C. |
|
| D. |
|
On complete combustion of an organic compound gave
of carbon dioxide and
of water. The percentage of carbon in the given organic compound is ______________.(Nearest Integer)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
CNG is an important transportation fuel. When CNG is mixed with
oxygen in vehicles, it leads to the formation of
and
and produces large quantity of heat during this combustion, then the amount of carbone dioxide, produced in grams is ____. [nearest integer]
| A. |
|
| B. |
|
| C. |
|
| D. |
|
116g of a substance upon dissociation reaction, yields 7.5g of hydrogen, 60g of oxygen and 48.5g of carbon. Given that the atomic masses of H,O and C are 1,16 and 12, respectively. The data agrees with how many formulae of the following?
_______________.
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The complete combustion of 0.492 g of an organic compound containing 'C', 'H' and 'O' gives 0.793g of . The percentage of oxygen composition in the organic compound is __________.(nearest integer)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Production of iron in a blast furnace follows the following equation
when are allowed to react then the amount of iron (in g) produced is:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
of nitrogen gas is mixed with excess of hydrogen gas and it is found that
of ammonia gas is produced. The volume of unused nitrogen gas is found to be ___
| A. |
|
| B. |
|
| C. |
|
| D. |
|
In the given reaction,
if one mole of each of X and Y with 0.05 mol of Z gives compound . (Given : Atomic masses of X, Y and Z are 10,20 and 30 amu, respectively.) The yield of
is ____________
.(Nearest integer)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Considering the above reaction, the limiting reagent of the reaction and the number of moles formed respectively are :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Consider the reaction The amount of
required to produce
of
is
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Consider the complete combustion of butane, the amount of butane utilized to produce of water is________
. (in nearest integer)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
of propane is completely reacted with
of oxygen. The mole fraction of carbon dioxide in the resulting mixture is
. The value of
is____________.(Nearest integer)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
A sample of a hydrate of barium chloride weighing 61 g was heated until all the water of hydration is removed. The dried sample weighed 52 g. The formula of the hydrated salt is : (atomic mass, Ba=137 amu, Cl=35.5 amu)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
If we have 1 mole of P and 3 mole of Cl2, which one is the limiting reagent and how many moles of PCl3 are formed?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
A sample of $\mathrm{NaClO}_3$ is converted by heat to NaCl with a loss of 0.16 g of oxygen. The residue is dissolved in water and precipitated as AgCl . The mass of AgCl (in g ) obtained will be : (Given: Molar mass of $\mathrm{AgCl}=143.5 \mathrm{gmol}_{-1}$ )
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The ratio of the masses percentages of and
of a saturated acyclic organic compound
are 4:1 and 3:4 respectively . Then , the moles of oxygen gas required for complete combustion of two moles of organic compound
is_____________
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The above reaction is carried out in a vessel starting with partial pressure . When the reaction is complete, the total pressure in the reaction vessel is _____m bar. (Round off of the nearest integer).
| A. |
|
| B. |
|
| C. |
|
| D. |
|
In bromination of Propyne, with Bromine 1,1,2,2-tetrabromopropane is obtained in $27 \%$ yield. The amount of $1,1,2,2$-tetrabromopropane obtained from 1 g of Bromine in this reaction is ........$\qquad$ $\times 10^{-1}$ g. (Nearest integer)
$($ Molar Mass : Bromine $=80 \mathrm{~g} / \mathrm{mol})$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
A 1.84 mg sample of polyhydric alcoholic compound ${ }^{\prime} X^{\prime}$ of molar mass $92.0 \mathrm{~g} / \mathrm{mol}$ gave 1.344 mL of $\mathrm{H}_2$ gas at STP. The number of alcoholic hydrogens present in compound ' X ' is _______________.
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The molecular formula of a commercial resin used for exchanging ions in water softening is C8H7SO3Na (Mol. wt. 206). What would be the maximum uptake of Ca2+ ions by the resin when expressed in mole per gram resin?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
3 g of activated charcoal was added to 50 mL of acetic acid solution (0.06N) in a flask. After an hour it was filtered and the strength of the filtrate was found to be 0.042 N. The amount of acetic acid (in mg) adsorbed (per gram of charcoal) is:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
What is ?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
How many moles of water are obtained when 3 moles of H2 react with 1 mole of O2?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The molecular formula of a commercial resin used for exchanging ions in water softening is $\mathrm{C}_8 \mathrm{H}_7 \mathrm{SO}_3 \mathrm{Na}$ (Mol. wt. 206). What would be the maximum uptake of $\mathrm{Ca}^{2+}$ ions by the resin when expressed in mole per gram resin?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The volume (in ml) of 0.125 M $\mathrm{AgNO}_3$ required to quantitatively precipitate chloride ions in 0.3g of $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right] \mathrm{Cl}_3$ is:
Molecular Mass of $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right] \mathrm{Cl}_3=267.46 \mathrm{~g} / \mathrm{mol}$
Molecular Mass of $\mathrm{AgNO}_3=169.87 \mathrm{~g} / \mathrm{mol}$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The electrophile, $E^{\oplus}$ attacks the benzene ring to generate the intermediate $\sigma$ - complex. Of the following, which $\sigma$-complex is of lowest energy?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
$\mathrm{Mg}+2 \mathrm{HCl} \rightarrow \mathrm{MgCl}_2+\mathrm{H}_2$
If 0.3 moles of Mg are added to a HCl container having 0.5 moles of HCl, how many moles of H2 are produced ____ $\times$10−2
| A. |
|
| B. |
|
| C. |
|
| D. |
|
For per gram of reactant taken, the maximum quantity of N2 gas is produced in which of the following thermal decomposition reactions ?
(Given : Atomic wt. - Cr=52u, Ba=137u)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
A bottle of soft drink has
dissolved in it. Assuming
behaves as an ideal gas, the volume of the dissolved
at STP is_____
. (Nearest integer)
Given : At STP, molar volume of an ideal gas is
| A. |
|
| B. |
|
| C. |
|
| D. |
|
When a hydrocarbon A undergoes complete combustion it requires 11 equivalents of oxygen and produces 4 equivalents of water. What is the molecular formula of A ?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Assume carbon burns according to the following equation :
When 12 g carbon is burnt in 48 g of oxygen, the volume of carbon monoxide produced is
STP [nearest integer]
[Given: Assume co as an ideal gas, the Mass of c is 12 g mol–1, the Mass of O is 16 g mol–1, and the molar volume of an ideal gas STP is 22.7 L mol–1]
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The above reaction was studied at by monitoring the concentration of
in which initial concentration was
and after half an hour became
. The rate of production of
is______
mol
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Find out the molarity of the compounds present in the final solution obtained on complete precipitation reaction between of
and
of
| A. |
|
| B. |
|
| C. |
|
| D. |
|
1.45 g of $\mathrm{P}_4$ was treated with 5.07 g of $\mathrm{O}_2$. Calculate the mass of $\mathrm{P}_4 \mathrm{O}_{10}$ formed in the given mixture:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
$4 \mathrm{P}_4+5 \mathrm{S}_8 \longrightarrow 4 \mathrm{P}_4 \mathrm{~S}_{10}$
If $31 \mathrm{~g}$ of $\mathrm{P}_4 \& 64 \mathrm{~g} \;of \mathrm{~S}_8$ react according to given equation then Limiting reagent is: $\left[{ }^{31} \mathrm{P},{ }^{32} \mathrm{S}\right]$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
$\mathrm{X}$ of ethanamine was subjected to reaction with $\mathrm{NaNO}_2 / \mathrm{HCl}$ followed by hydrolysis to liberate $\mathrm{N}_2$ and $\mathrm{HCl}$. The $\mathrm{HCl}$ generated was completely neutralised by 0.2 moles of $\mathrm{NaOH} . \mathrm{X}$ is______g.
| A. |
|
| B. |
|
| C. |
|
| D. |
|
$1 \mathrm{~L}, 0.02 \mathrm{M} {\text {solution of }}\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5 \mathrm{SO}_4\right] \mathrm{Br }, {\text {is mixed with }} 1 \mathrm{~L}, 0.02 \mathrm{M}$ solution of $\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_5 \mathrm{Br}\right] \mathrm{SO}_4$. The resulting solution is divided into two equal parts $(\mathrm{X})$ and treated with excess of $\mathrm{AgNO}_3$ solution and $\mathrm{BaCl}_2$ solution respectively as shown below:
1 L solution $(\mathrm{X})+\mathrm{AgNO}_3$ solution (excess) $\rightarrow \mathrm{Y}$
1 L solution $(\mathrm{X})+\mathrm{BaCl}_2$ solution (excess) $\rightarrow \mathrm{Z}$
The number of moles of $Y$ and $Z$ respectively are
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Given the reaction
$2 \mathrm{~N}_2+3 \mathrm{H}_2 \rightleftharpoons 2 \mathrm{NH}_3$
How many grams of $\mathrm{NH}_3$ will be produced when 56 g of $\mathrm{N}_2$ burnt?
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Identify the incorrect statements regarding primary standard of titrimetric analysis
(A) It should be purely available in dry form.
(B) It should not undergo chemical change in air.
(C) It should be hygroscopic and should react with another chemical instantaneously and stoichiometrically.
(D) It should be readily soluble in water.
(E) $\mathrm{KMnO}_4 \& \mathrm{NaOH}$ can be used as primary standard.
Choose the correct answer from the options given below :
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Identify the limiting Reagent in the following reactions
$\mathrm{CH}_4(\mathrm{~g})+2 \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Given below are some nitrogen-containing compounds.
Each of them is treated with HCl separately. 1.0 g of the most basic compound will consume
$\qquad$___ mg of HCl .
(Given molar mass in $\mathrm{g} \mathrm{mol}^{-1} \mathrm{C}: 12, \mathrm{H}: 1, \mathrm{O}: 16$, $\mathrm{Cl}: 35.5)$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The molar mass of the water insoluble product formed from the fusion of chromite ore $\left(\mathrm{FeCr}_2 \mathrm{O}_4\right)$ with $\mathrm{Na}_2 \mathrm{CO}_3$ in presence of $\mathrm{O}_2$ is $\qquad$___$\mathrm{g} \mathrm{mol}^{-1}$.
| A. |
|
| B. |
|
| C. |
|
| D. |
|
A solution of 20.2 g of 1,2-dibromopropane in MeOH upon heating with excess $Z n$ produces 3.58 g of an unsaturated compound $\mathbf{X}$. The yield (%) of $\mathbf{X}$ is closest to
[Atomic weight of $B r$ is 80 ]
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The amount of metallic Zn(in g) whose atomic weight is 65.4 required to react with aqueous sodium hydroxide to produce 1 kg of $\mathrm{H}_2$ is
| A. |
|
| B. |
|
| C. |
|
| D. |
|
$\mathrm{CaCO}_3(\mathrm{~s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{CaCl}_2(\mathrm{aq})+\mathrm{CO}_2(\mathrm{~g}) \mathrm{H}_2 \mathrm{O}(\mathrm{l})$
Consider the above reaction, what mass of $\mathrm{CaCl}_2$ will be formed if 250 mL of 0.76 M HCl reacts with 1000 g of $\mathrm{CaCO}_3$ ?
(Given : Molar mass of $\mathrm{Ca}, \mathrm{C}, \mathrm{O}, \mathrm{H}$ and Cl are 40 , $12,16,1$ and $35.5 \mathrm{~g} \mathrm{~mol}^{-1}$, respectively)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
X g of nitrobenzene on nitration gave 4.2 g of m -dinitrobenzene.
X = ___________ g. (nearest integer)
[Given : molar mass (in $\mathrm{g} \mathrm{mol}^{-1}$ ) $\mathrm{C}: 12, \mathrm{H}: 1$, $\mathrm{O}: 16, \mathrm{~N}: 14]$
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Phosphorus and oxygen are heated together in a closed vessel to form $\mathrm{P}_2 \mathrm{O}_3$ and $\mathrm{P}_2 \mathrm{O}_5$ in a molar ratio of 2 : 1 respectively. The mass of oxygen taken is three times the mass of phosphorus. Assuming phosphorus reacts in its monoatomic form and that the limiting reactant is completely consumed, answer the following:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
When 22.4 litres of H2(g) is mixed with 11.2 litres of Cl2(g), each at S.T.P, the moles of HCl(g) formed is equal to ____mol of HCl (g)
| A. |
|
| B. |
|
| C. |
|
| D. |
|
10 g of hdyrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction ( in mol) will be -
| A. |
|
| B. |
|
| C. |
|
| D. |
|
The number of moles of hydrogen molecules required to produce 20 moles of ammonia through Haber's process is:
| A. |
|
| B. |
|
| C. |
|
| D. |
|
Stoichiometry deals with the calculation of masses of the reactants and the products involved in a chemical reaction.
