Limiting Reagent or Reactant

Q. What information does the following chemical equation convey?​
$\mathrm{Zn}+H_2{\mathrm{SO}}_4\to {\mathrm{ZnSO}}_4+H_2$

Q.

Under similar conditions of pressure and temperature, 40 ml of slightly moist hydrogen chloride gas is mixed with 20 ml of ammonia gas, the final volume of gas at the same temperature and pressure will be

1. 100 ml
2. 20 ml
3. 40 ml
4. 60 ml

Q. $10g$ of hydrogen and $64g$ of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be:

1. $3moles$
2. $4moles$
3. $1moles$
4. $2moles$

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. 1/3

3. 0.125

4. 0.5

Q. When 3 g of carbon is burnt in 8 g oxygen, 11 g of carbon dioxide is produced. Will the amount of carbon dioxide increase if 3 g of carbon is now burnt in 50 g of oxygen?
Which law of chemical combinations will govern your answer?

Q. How many moles of methane are required to produce $22g{CO}_2\left(g\right)$ after combustion?

Q. What are five types of salts? Explain with examples.

Q.

A+B$⟶$$A_3{B}_2$(unbalanced)$A_3{B}_2$+C$⟶$$A_3{B}_2{C}_2$(unbalanced)

Above two reactions are carried out by taking 3 moles each of A and B and one mole of C. Then which option is wrong

1. 1 mole of A₃B₂C₂ is formed

2. 1/2 mole of A₃B₂C₂ is formed

3. 1 mole of A₃B₂ is formed

4. 1/2 mole of A₃B₂ is left finally

Q. Calculate number of moles of ${Na}_2{SO}_4$ produced from 1 mole of $NaOH$
$2NaOH+H_2{SO}_4\to {Na}_2{SO}_4+2H_{2}O$

Q. Initial volume of a gas is 1 L at temperature 100 K. What is the volume of a gas at 300 K.

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

Q. If 12 g of alkaline earth metal gives 14.8 g of its nitride, then what is the atomic weight of metal?

1. 12
2. 20
3. 40
4. 14.8

Q.

If $0.5mole$ of $BaC{l}_2$ is mixed with $0.2mole$ of $N{a}_{3}P{O}_4$, the maximum number of moles of $B{a}_3(P{O}_4{)}_2$ formed are

1. 0.5

2. 0.3

3. 0.7

4. 0.1

Q. Maximum number of moles of potash alum $K_{2}S{O}_{4}A{l}_2(S{O}_4{)}_3$ can be made from sample of aluminum-containing $5.4g$ of aluminium (considerning 100% yield) is?

1. ${10}^{-2}$ mole
2. $0.1$ mole
3. $0.5\times {10}^{-2}$ moles
4. $0.2$ moles

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. What should be the weight and moles of AgCl precipitate obtained on adding 500ml of 0.20 M HCl in 30 g of $AgN{O}_3$ solution? $(AgN{O}_3=170)$

1. 14.35 g
2. 15 g
3. 18 g
4. 19 g

Q.

18g of steam is passed over 2g of Iron.$H_{2}O+Fe\to H_2+F{e}_2{O}_3$ Which is the excessive reagent? [Fe = 55.85g]

1. 

2. 

3. 

4. 

Q. Which of the following has the smallest number of molecules?

1. $22$ g of $C{O}_2$ gas
2. $11.2$ L of $C{O}_2$ gas
3. $0.1$ mole of $C{O}_2$ gas
4. $22.4\times {10}^3$ mL of $C{O}_2$ gas

Q. When calcium oxide is dissolved in water calcium hydroxide is formed. Which law of the following law is obeyed here?

1. Law of constant proportion
2. Law of conservation of mass
3. Law of Multiple proportion
4. None of these

Q.

In each of the following questions, an Assertion (A) is followed by a corresponding Reason (R). Use the following keys to choose the appropriate answer.

Assertion (A): If 30 mL of $H_2$ and 20 mL of $O_2$ react to form water, 5 mL of $H_2$ is left at the end of the reaction.
Reason (R): $H_2$ is the limiting reagent.

1. If both (A) and (R) are correct and (R) is the correct explanation for (A).

2. If both (A) and (R) are correct and (R) is not the correct explanation for (A).

3. If (A) is correct but (R) is incorrect.

4. If (A) is incorrect and (R) is correct.

5. If both (A) and (R) are incorrect.

Q. One mole of the compound on treating with an excess of aq.$AgN{O}_3$. The number of moles of $AgCl$ formed will be:

1. 0
2. 1
3. 2
4. 3
5. 4
6. 5
7. 6
8. 7
9. 8
10. 9

Q. Mass of reactants is always equal to the mass of the products. (Don't consider nuclear reaction)

1. True
2. False

Q. In the following reaction, at $STP$, how many liters of $S{O}_2$ will require to burn completely a pure sulfur in $8$ litres of oxygen?
$S\left(s\right)+O_2\left(g\right)\to S{O}_2\left(g\right)$

1. $1$
2. $4$
3. $8$
4. $16$
5. $32$

Q.

$2VO+3F{e}_2{O}_3\to 6FeO+V_2{O}_5$ If we start with 2g of VO and 5.75g of $F{e}_2{O}_3$, which is the limiting reagent?

[V = 47.87g] [Fe = 55.85g]

1. VO

2. 

3. 

4. 

Q. An electric discharge is passed through a mixture containing 50 c.c. of $O_2$ and 50 c.c. of $H_2$. The volume of the gases formed (i) at room temperature and (ii) at 110⁰C will be

1. (i) 25 c.c. (ii) 50 c.c.
2. (i) 50 c.c. (ii) 75 c.c.
3. (i) 25 c.c. (ii) 75 c.c.
4. (i) 75 c.c. (ii) 75 c.c.

Q.

30 mL of hydrogen and 20 mL of oxygen react to give water. What is left at the end of the reaction?

1. 5 mL of oxygen

2. 10 mL of hydrogen

3. 5 mL of hydrogen

4. 10 mL of oxygen

Q.

Is 400g of oxygen gas enough to burn 20 moles of methane completely?

1. Yes

2. No

3. All the above

4. Insufficient data

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. The reaction
$C{l}_2+S_2{O_3}^{2-}+{OH}^{-}⟶{{SO}_4}^{2-}+{Cl}^{-}+H_{2}O$
Starting with $0.15$ mole $C{l}_2,0.010$ mole$S_2{O_3}^{2-}$and $0.30$ mole ${OH}^{-}$, mole of $C{l}_2$ left in solution will be

1. 0.09
2. 0.11
3. 0.01
4. 0.04

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

Q. If $1$ stands for true and $0$ stands for false, then choose the correct code for the following statement:
End point in the titration of $CuS{O}_4$ iodometrically (with starch as the indicator) is the disappearance of blue color.