﻿ 1.0 g of magnesium is burnt with 0.56 g of O2 in a closed vessel. Which reactant is left in excess and how much? from Chemistry Some Basic Concepts of Chemistry Class 12 Nagaland Board

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Equal masses of H2, O2 and methane have been taken in a container of volume V at temperature 270 C in identical conditions. The ratio of the volumes of gases H2 : O2: CH4 would be

• 8:16:1

• 16:8:1

• 16:1:2

• 8:1:2

C.

16:1:2

Volume of a gas (V)  number of moles (n)
Therefore, the ratio of the volumes of gases can be determined in terms of their moles. The ratio of volumes of H2:O2: methane (CH4) is given by

Volume of a gas (V)  number of moles (n)
Therefore, the ratio of the volumes of gases can be determined in terms of their moles. The ratio of volumes of H2:O2: methane (CH4) is given by

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# 1.0 g of magnesium is burnt with 0.56 g of O2 in a closed vessel. Which reactant is left in excess and how much? Mg, 0.16 g O2, 0.16 g Mg, 0.44 g O2, 0.28 g

A.

Mg, 0.16 g

The balanced chemical equation is
Mg + 1/2O2 --> MgO
24g    16 g        40g

From the above equation, it is clear that,
24 f Mg reacts with 16 g O2
thus, 1.0 g Mg reacts with

The balanced chemical equation is
Mg + 1/2O2 --> MgO
24g    16 g        40g

From the above equation, it is clear that,
24 f Mg reacts with 16 g O2
thus, 1.0 g Mg reacts with

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6.02 x 1020 molecules of urea are present in 100 mL of its solution. The concentration of solution is

• 0.02 M

• 0.01 M

• 0.001 M

• 0.1 M

B.

0.01 M

Given, number of molecules of urea =6.02 x 1020
therefore ,Number of moles

Given, number of molecules of urea =6.02 x 1020
therefore ,Number of moles

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When 22.4 L of H2 (g) is mixed with 11.2 L of Cl2 (g), each of at STP, the moles of HCl (g) formed is equal to

• 1 mole of HCl (g)

• 2 moles of HCl (g)

• 0.5 mole of (g)

• 1.5 mole of HCl(g)

A.

1 mole of HCl (g)

The given problem is related to the concept of the stoichiometry of chemical equations. Thus, we have to convert the given volumes into their moles and then identify the limiting reagent [possessing minimum number of moles and completely used up in the reaction]
The limiting reagent gives the moles of product formed in the reaction.

The given problem is related to the concept of the stoichiometry of chemical equations. Thus, we have to convert the given volumes into their moles and then identify the limiting reagent [possessing minimum number of moles and completely used up in the reaction]
The limiting reagent gives the moles of product formed in the reaction.

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Equal moles of hydrogen and oxygen gases are placed in a container with a pin-hole through which both can escape. What fraction of the oxygen escapes in the time required for one-half of the hydrogen to escape?

• 1/4

• 3/8

• 1/2

• 1/8

D.

1/8

we have given,
a number of moles of hydrogen and that of oxygen are not equal.

we have given,
a number of moles of hydrogen and that of oxygen are not equal.

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