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1.	How many molecules are present in 4.9g of H2SO4?
Answer» For H₂SO₄ one mole is equal to 98 grams. Therefore, calculating the number of moles for 4.9 grams n = 4.9/98 = 0.05 moles So, for 0.05 moles the number of gram molecules is 0.05-gram molecules. Hence, the number of gram molecules is 0.05.

How many molecules are present in 4.9g of H2SO4?

Answer»

For H₂SO₄ one mole is equal to 98 grams.

Therefore, calculating the number of moles for 4.9 grams

n = 4.9/98 = 0.05 moles

So, for 0.05 moles the number of gram molecules is 0.05-gram molecules.

Hence, the number of gram molecules is 0.05.

Discussion

2.	what is the character of coordinate covalent molecule
Answer» In coordinate bonding, the donor is the atom that shares a pair of electrons from itself to the other atom. The acceptor or receptor is the atom that receives the electron pair shared by the donor to attain stability.

Discussion

3.	Please find the question in the image below.The correct answer is (2) 80. Please explain the solution.
Answer» a(initial) =10 M ....> 80% changed into product \(a(t)=10(10*80/100)= 2M\) If a₀= 5 M , In the same time duration same percentage of initial concentration changes into products because in first order reaction is independent from initial concentration.

Discussion

4.	4 g of carbon was heated with 8 grams of Sulphur. How much CS2 was formed when the reaction is completed. Find out the amount of reactant left unreacted.
Answer» \(4C + S_8 \rightarrow 4CS_2\) \(\therefore \) Number of moles of carbon = \(\frac 4{12} = 0.33 \,mol\) Number of moles of sulphur = \(\frac 8{256.8} = 0.031\, mol\) \(\because \) 1 mole of S₈ react with = 4 mole of carbon \(\therefore \) \(\)0.031 mole of S₈ react with = (4 x 0.031) mole of carbon = 0.12 mol of carbon but we have 0.33 moles of carbon \(\therefore \) S₈ is a limiting reagent. \(\therefore \) Number of moles of CS₂ formed = 0.031 x 4 \(\therefore \) Weight of CS₂ = 0.031 x 4 x 76 = 9.42 g Number of moles of carbon left = 0.33 - 0.12 = 0.21 mol or = 0.21 x 12 g = 2.52 g Hence, 9.42 g CS₂ will formed and 2.52 g carbon left unreacted.

4 g of carbon was heated with 8 grams of Sulphur. How much CS2 was formed when the reaction is completed. Find out the amount of reactant left unreacted.

Answer»

\(4C + S_8 \rightarrow 4CS_2\)

\(\therefore \) Number of moles of carbon = \(\frac 4{12} = 0.33 \,mol\)

Number of moles of sulphur = \(\frac 8{256.8} = 0.031\, mol\)

\(\because \) 1 mole of S₈ react with = 4 mole of carbon

\(\therefore \) \(\)0.031 mole of S₈ react with = (4 x 0.031) mole of carbon

= 0.12 mol of carbon

but we have 0.33 moles of carbon

\(\therefore \) S₈ is a limiting reagent.

\(\therefore \) Number of moles of CS₂ formed = 0.031 x 4

\(\therefore \) Weight of CS₂ = 0.031 x 4 x 76 = 9.42 g

Number of moles of carbon left = 0.33 - 0.12 = 0.21 mol

= 0.21 x 12 g

= 2.52 g

Hence, 9.42 g CS₂ will formed and 2.52 g carbon left unreacted.

Discussion

Explore topic-wise InterviewSolutions in .

How many molecules are present in 4.9g of H2SO4?

what is the character of coordinate covalent molecule

Please find the question in the image below.The correct answer is (2) 80. Please explain the solution.

a(initial) ​=10 M ....> 80% changed into product

If a0 = 5 M , In the same time duration same percentage of initial concentration changes into products because in first order reaction is independent from initial concentration.

4 g of carbon was heated with 8 grams of Sulphur. How much CS2 was formed when the reaction is completed. Find out the amount of reactant left unreacted.

a(initial) =10 M ....> 80% changed into product

If a₀= 5 M , In the same time duration same percentage of initial concentration changes into products because in first order reaction is independent from initial concentration.