MABS Institution
11th Chemistry Monthly Test - 1 ( Basic Concepts of Chemistry and Chemical Calculations )-Aug 2020
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Calculate the average atomic mass of naturally occurring magnesium using the following data
Isotope Istopic atomic mass Abundance(%) Mg24 23.99 78.99 Mg26 24.99 10.00 Mg25 25.98 11.01 -
The density of carbon dioxide is equal to 1.965 kgm-3 at 273 K and 1 atm pressure. calculate the molar mass of CO2
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Calculate the molar mass of the following compounds. -boric Acid [H3BO3]
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Balance the following equations by ion electron method \(Zn+{ NO }_{ 3 }^{ - }\longrightarrow { Zn }^{ 2+ }+No\)
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Calculate the number of atoms/molecules present in the following 1.8g of water
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Calculate equivalent mass of the Magnesium hydroxide
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How are 0.5 mol Na2CO3 and 0.50 M Na2CO3 different?
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In a reaction x + y + Z2 \(\longrightarrow \) xyz2 identify the Limiting reagent if any, in the following reaction mixtures.
(a) 200 atoms of x +200 atoms of y + 50 molecules of z2
(b) 1 mol of x + 1 mol of y + 3 mol of z2
(c) 50 atoms of x + 25 atoms of y + 50 molecules of z2
(d) 2.5 mol of x + 5 mol of y + 5 mol of z2 -
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State Avogadro's hypothesis.
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Calculate the mass of the following: 1 atom of silver
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Calculate the gram molecular mass of sugar having molecular formula C12H22O11
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The density of CO2 =1.977kgm-3 at STP. Calculate I the molecular mass of CO2
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Calculate the equivalent mass of bicarbonate ion.
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Define atomicity.
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In a reaction, A + B2 \(\longrightarrow \) AB2, identify the limiting reagent if any in the following reaction mixtures
(i) 300 atoms of A + 200 molecules of B
(ii) 2 moles of A + 3 moles of B
(iii) 100 atoms of A + 100 molecules of B
(iv) 5 moles of A + 2.5 moles of B
(v) 2.5 moles of A + 5 moles of B -
Balance the following equations by ion electron method -
i) \({ KMn }O_{ 4 }+{ SnCl }_{ 2 }+HCI\longrightarrow MnCI_{ 2 }+{ SnCI }_{ 4 }+{ H }_{ 2 }O+KCI\)
ii) \({ C }_{ 2 }{ O }_{ 4 }^{ 2- }+{ Cr }_{ 2 }{ O }_{ 7 }^{ 2- }\longrightarrow { Cr }^{ 3+ }+{ CO }_{ 2 }\) (in acid medium)
iii) \({ Na }_{ 2 }{ S }_{ 2 }{ O }_{ 3 }+{ I }_{ 2 }\longrightarrow { Na }_{ 2 }{ S }_{ 4 }{ O }_{ 6 }+NaI\)
iv) \(Zn+{ NO }_{ 3 }^{ - }\longrightarrow { Zn }^{ 2+ }+No\) -
Calculate the molar mass of the following compounds. -
i) urea [CO(NH2)2]
ii) acetone [CH3 COCH3]
iii) boric Acid [H3BO3]
iv) Sulphurci Acid [H2SO4] -
Write note on decomposition reaction
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Explain displacement reaction.
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Arrange the elements silver, Zinc and copper in the order of their decreasing electron releasing tendency and justify your arrangement with an appropriate experiment.
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The reaction between aluminum and ferric oxide can generate temperatures up to 3273 K and is used in welding metals. (Atomic mass of AC = 27 u atomic mass of O = 16 u )
2Al + Fe2O3 \(\longrightarrow \) Al2O3 + 2Fe; If in this process, 324 g of aluminum is allowed to react with 1.12 kg of ferric oxide
i) Calculate the mass of Al2O3 formed
ii) How much of the excess reagent is left at the end of the reaction? -
Write note on combination reaction.
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Distinguish between the following.
(i) Atomic and molecular mass
(ii) Atomic mass and atomic weight
(iii) Empirical and molecular formula
(iv) Moles and molecules. -
Balance the following equations by oxidation number method
i) \({ K }_{ 2 }{ Cr }_{ 2 }{ O }_{ 7 }+KI+{ H }_{ 2 }SO_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+{ Cr }_{ 2 }({ SO }_{ 4 })+{ I }_{ 2 }+{ H }_{ 2 }O\)
ii) \({ K }Mno_{ 4 }+{ Na }_{ 2 }{ So }_{ 3 }\longrightarrow { MnO }_{ 2 }+{ Na }_{ 2 }{ So }_{ 4 }+KOH\)
iii) \(Cu+{ HNO }_{ 3 }\longrightarrow Cu\left( { NO }_{ 3 } \right) _{ 2 }+{ NO }_{ 2 }+{ H }_{ 2 }O\)
iv) \({ KMn }O_{ 4 }+{ H }_{ 2 }{ C }_{ 2 }{ O }_{ 4 }+{ H }_{ 2 }{ SO }_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+{ MnSO }_{ 4 }+{ CO }_{ 2 }+{ H }_{ 2 }O\)