Limiting Reagent or Reactant

Q. What is the molarity of a 4.9% $H_{3}P{O}_4$ solution by mass? (Density of $H_{3}P{O}_4$ solution = 1.22 g/mL)?

1. 0.61 M
2. 0.05 M
3. 1.22 M
4. 1.54 M

Q. 0.5 moles of $H_{2}S{O}_4$ is mixed with 0.2 moles of $Ca(OH{)}_2.$ The maximum number of moles of $CaS{O}_4$ formed is:
Reaction: $H_{2}S{O}_4+Ca(OH{)}_2\to CaS{O}_4+2H_{2}O$

1. 0.2 mol
2. 0.5 mol
3. 0.4 mol
4. 1.5 mol

Q. How many moles of $Zn[Fe{S}_2{]}_2$ can be made from 2 g of $Zn$, 3 g of $Fe$ and 4 g of $S$?
$Zn+2Fe+4S\to Zn[Fe{S}_2{]}_2$
(Given: Molar mass of $Fe$ = 56 g/mol and molar mass of $Zn$ = 65 g/mol)

1. 0.0157 mol
2. 0.0265 mol
3. 0.2650 mol
4. 0.0538 mol

Q.

$1.2\mathrm{g}$ of $\mathrm{Mg}$ (At Mass 24) will produce $\mathrm{MgO}$ equal to?

Q. At STP, the volume of ammonia formed using 1 mole of nitrogen and 4 moles of hydrogen on complete reaction is:

1. 67.2 L
2. 11.2 L
3. 22.4 L
4. 44.8 L

Q. Consider the following balanced reaction:
$2Ca\left(s\right)+O_2\left(g\right)\to 2CaO$
If 60 g of Ca is placed in a reaction chamber with 32 g of $O_2,$ which will be the limiting reactant and mass of the excess reactant left?

1. Calcium; 8 g
2. Oxygen; 8 g
3. Oxygen; 16 g
4. Calcium; 10 g

Q. 10 g of Hydrogen and 64 g of Oxygen were filled in a steel vessel and exploded. Calculate the amount of water produced in the reaction.

1. 5 mol
2. 3 mol
3. 2 mol
4. 4 mol

Q. Consider the following reaction:
$8Fe+S_8\to 8FeS$
If we begin with 293 g of Fe and 17.2 g of $S_8$, how many grams of FeS will be produced?

1. 42.30 g
2. 45.00 g
3. 52.03 g
4. 47.17 g

Q. How many moles of $H_2$ will be needed to produce 6 moles of $H_{2}O$ when it reacts with excess of $O_2$ ?

1. 3
2. 4
3. 6
4. 5

Q. If $27\text{g}$ of carbon is mixed with $88\text{g}$ of oxygen and is allowed to burn to produce $C{O}_2$, then:

1. Oxygen is the limiting reagent
2. Volume of $C{O}_2$ gas produced at NTP is $50.4\text{L}$
3. $C$ and $O$ combine in mass ratio $3:8$
4. Volume of unreacted $O_2$ at STP is $11.2\text{L}$

Q. For the reaction,
$2H_2\left(g\right)+O_2\left(g\right)\to 2H_{2}O\left(g\right)$
Initially, 3 moles of $H_2$ and 2 moles of $O_2$ are present. Identify the correct statement.

1. $H_2$ is the limiting reagent
2. $O_2$ is the limiting reagent
3. 1 mol of $H_2$ is left unreacted
4. 1 mol of $O_2$ is left unreacted

Q. How many grams of titanium (IV) oxide can be produced when 80 g of $TiC{l}_4$ is made to react with 20 g of $O_2$ as shown in the following equation? (Molar mass of titanium = 48 g/mol)
$TiC{l}_4\left(s\right)+O_2\left(g\right)\to Ti{O}_2\left(s\right)+2C{l}_2\left(g\right)$

1. 130 g
2. 34 g
3. 50 g
4. 88 g

Q. Calculate the number of moles of $F{e}_2{O}_3$ when 600 g of $Fe{S}_2$, reacts with 800 g of $O_2.$
$4Fe{S}_2+11O_2\to 2F{e}_2{O}_3+8S{O}_2$
(Given: Molar mass of Fe is 56 g/mol)

1. 1 mol
2. 1.5 mol
3. 2 mol
4. 2.5 mol

Q.

The number of moles of $F{e}_2{O}_3$ formed when $0.5moles$ of $O_2$ and $0.5moles$ of $Fe$ are allowed to react are

1. 0.25

2. 0.5

3. $\frac{1}{3}$

4. 0.125

Q. The ratio of amounts of $H_{2}S$ needed to precipitate all the metal ions from 100 ml of 1 M $AgN{O}_3$ and 100 ml of 1 M $CuS{O}_4$ will be

1. 1 : 1
2. 1 : 2
3. 2 : 1
4. None of these

Q. Law of multiple proportions is not applicable for the oxide(s) of:

1. Aluminium
2. Iron
3. Nitrogen
4. Carbon

Q. Sodium azide $\left(Na{N}_3\right)$ is an explosive chemical used in automobile airbags. It is made by the following reaction:
$NaN{O}_3+3NaN{H}_2\to Na{N}_3+3NaOH+N{H}_3$

One takes 17.0 g of $NaN{O}_3$ and 13.0 g of $NaN{H}_2$. If this amount is used in automobile bags, how much $N_2$ is formed due to collision at STP?

1. 3.73 L
2. 12.93 L
3. 8.62 L
4. 2.15 L

Q. Find the moles of HCl gas obtained at STP from the following set of reactions:
$FeC{l}_3+O_2\to F{e}_2{O}_3+C{l}_2\left(g\right)H_2\left(g\right)+C{l}_2\left(g\right)\to 2HCl\left(g\right)$
Starting with 4.56 mol of $FeC{l}_3$ , 33.6 L of $O_2$ at STP and 7 mol of $H_2$ gas.
(Molar mass of Fe = 56 g/mol)

1. 2 mol
2. 6 mol
3. 4 mol
4. 8 mol

Q. Consider the following balanced reaction:
$2Ca\left(s\right)+O_2\left(g\right)\to 2CaO$
If 60 g of Ca is placed in a reaction chamber with 32 g of $O_2,$ which will be the limiting reactant and mass of the excess reactant left?

1. Calcium; 8 g
2. Oxygen; 16 g
3. Calcium; 10 g
4. Oxygen; 8 g

Q. Assertion: When 4 moles of $H_2$ react with 2 moles of $O_2$, then 4 moles of water is formed.
Reason: $O_2$ will act as the limiting reagent

1. Both the assertion and the reason are true, and the reason is the correct explanation of the assertion.
2. Both the assertion and the reason are true, but the reason is not the correct explanation of the assertion.
3. The assertion is true, but the reason is false.
4. Both the assertion and the reason are false statements.

Q. 0.006 moles of $Ca(N{O}_3{)}_2$ are added to an aqueous solution containing 0.003 moles of $N{a}_2{C}_2{O}_4$ and the reaction is allowed to go to completion. Select the incorrect statement from the following:

1. 0.003 mole of calcium oxalate will get precipitated.
2. 0.001 moles of $C{a}^{2+}$ will remain in excess.
3. $N{a}_2{C}_2{O}_4$ is the limiting reagent.
4. $Ca(N{O}_3{)}_2$ is the excess reagent.

Q. 6 moles of $N{a}_{2}C{O}_3$ is reacted with 10 moles of $HCl$. Find the volume of $C{O}_2$ gas produced at STP.
The reaction is:
$N{a}_{2}C{O}_3+2HCl\to 2NaCl+C{O}_2+H_{2}O$

1. $134.4\text{L}$

2. $112\text{L}$
3. $22.4\text{L}$
4. $44.8\text{L}$

Q.

16.8 litre gas containing $H_2$ and $O_2$ is formed at NTP on electrolysis of water. What should be the weight of electrolysed water

1. 5 g
2. 9 g
3. 10 g
4. 12 g

Q. If 200 ml of 0.3 M $H_{3}P{O}_3$ is mixed with 200 ml of 0.3 M $Ba(OH{)}_2$, find the incorrect option from the following:

1. $H_{3}P{O}_3$ is limiting reagent if the reaction goes to completion
2. Reactants get used up if $Ba\left(HP{O}_3\right)$ is the product
3. $H_{3}P{O}_3$ is the limiting reagent if $Ba(H_{2}P{O}_3{)}_2$ is the product
4. Reactants get used up if $Ba\left(OH\right)\left(H_{2}P{O}_3\right)$ is the product.

Q.

Reaction	Yield of the reaction
$\left(i\right)2A+3B\to 3C+D$	80%
$\left(ii\right)2C+E\to 4F$	40 %
$\left(iii\right)3F+7H\to 8G$	50%

Starting with 6 mol of A, 9 mol of B, 4 mol of E and 15 mol of H, the number of moles of G formed will be

1. 4.48 mol
2. 7.68 mol
3. 5.28 mol
4. 6.68 mol

Q. Suppose 316.0 g of aluminium sulphide reacts with 493.0 g of water, what mass of the excess reactant will remain?
Given reaction: $A{l}_2{S}_3+6H_{2}O\to 2Al(OH{)}_3+3H_{2}S$

1. 265.14 g
2. 108.52 g
3. 400 g
4. 66.25 g

Q. How many moles of oxygen is required to burn one mole of methane, completely ?

1. 1
2. 3
3. 2
4. 4

Q. Nitric acid is the most important oxi-acid formed by nitrogen. It is one of the major industrial chemicals and is widely used. Nitric acid is manufactured by the catalytic oxidation of ammonia that is known as Ostwald Process which can be represented by sequence of reactions shown below
$4N{H}_3+5O_2\left(g\right)\underset{Pt/Rh}{\overset{Catalyst}{\to }}4NO\left(g\right)+6H_{2}O\left(g\right)...\left(i\right)$
$2NO\left(g\right)+O_2\left(g\right)\stackrel{1120K}{\to }2N{O}_2\left(g\right)...\left(ii\right)$
$3N{O}_2\left(g\right)+H_{2}O\left(l\right)\to 2HN{O}_3\left(aq\right)+NO\left(g\right)...\left(iii\right)$
The aqueous nitric acid obtained by this method can be concenteated by distillation to $68.5\%$ by weight. Further concentration to $98\%$ acid can be achieved by dehydration with concentrated sulphuric acid.

$85kg$ of $N{H}_3\left(g\right)$ was heated with $320kg$ oxygen in the first step and $HN{O}_3$ is prepared according to the above reactions. If the final solution has volume $500L$, then molarity of $HN{O}_3$ is:

1. 2 M
2. 8 M
3. 3.33 M
4. 6.66 M

Q. 50.0 kg of $N_2\left(g\right)$ and 10.0 kg of $H_2\left(g\right)$ are mixed to produce $N{H}_3\left(g\right).$ Calculate the mass of $N{H}_3$(g) formed:

1. 40.0 kg
2. 14.0 kg
3. 25.0 kg
4. 56.6 kg

Q. A reaction container holds 5.77 g of $P_4$ and 5.77 g of $O_2$ and the following reaction occurs: $P_4+O_2\to P_4{O}_6.$ The amount of excess reagent left is?

1. 10.51 g
2. 2.84 g
3. 20.32 g
4. 1.31 g