CBSE Questions for Class 11 Medical Chemistry Some Basic Concepts Of Chemistry Quiz 3 - MCQExams.com

The molar mass of haemoglobin is about $$65000 \: g\:mol^{-1}$$. Every haemoglobin contains $$4 $$ iron atoms. Thus :
  • iron content in haemoglobin is $$0.35$$% by mass
  • $$1$$ mole of haemoglobin contains $$56$$g of iron
  • $$1$$ mole of haemoglobin contains $$224$$g of iron
  • if Iron content is increased to $$0.56$$%, molar mass of haemoglobin would be higher than $$65000 \: g\: mol^{-1}$$
Which pair has the same percentage of carbon?
  • $$CH_3COOH \: and \: C_6H_{12}O_6$$
  • $$CH_3COOH \: and \: C_{12}H_{22}O_{11}$$
  • $$CH_3COOH \: and \: C_2H_5OH$$
  • $$C_6H_{12}O_6 \: and \: C_{12}H_{22}O_{11}$$
In diammonium hydrogen phosphate, $$(NH_4)_2HPO_4$$, percentage of :
  • $$P_2O_5$$ is $$53.78$$%
  • $$NH_3$$ is $$25.76$$%
  • $$P$$ is maximum
  • $$N$$ is maximum
$$800$$ g of a $$40\%$$ solution by weight was cooled. $$100$$ g of solute was precipitated. The percentage composition of remaining solution is :
  • $$31.4\%$$
  • $$20.0\%$$
  • $$23.0\%$$
  • $$24\%$$
The volume occupied by 7 grams of nitrogen gas at STP is:
  • 6.5
  • 5.6
  • 7.5
  • 4.5
How many g of $$KCl$$ would have to be dissolved in $$60$$ g $${H}_{2}O$$ to give $$20\%$$ by mass of solution?
  • $$15$$ g
  • $$1.5$$ g
  • $$11.5$$ g
  • $$31.5$$ g
Atomic number (Z) of a neutral atom and mass number (A) of an atom are equal to: 
(Here n = number of neutrons and p = number of protons):
  • Z = n and A = n+p
  • Z = e and A = n+e
  • Z = p and A = n+p
  • Z = n and A = p+e
The average molar mass of air becomes more in presence of which gas if present in air :
  • $${H}_{2}$$
  • $${N}_{2}$$
  • $${C}_{2}{H}_{6}$$
  • $$C{H}_{4}$$
Find the weight of a substance if its molecular weight is $$70$$ and in the gaseous form it occupies $$10$$ L at $$27^oC$$ and $$760$$ mm $$Hg$$ pressure.
  • 32.5 g
  • 35.5 g
  • 28.38 g
  • None of the above
Which facts are revealed from Avogadro's law for ideal gases?
  • The distance between molecules is much large than the actual dimension of molecules.
  • Equal number of molecules of different gases under identical conditions of temperatures and pressure occupy the same volume.
  • Saturated vapours obey gas laws
  • 1 mole of a gas contains $$6.023\times 10^{23}$$ molecules of gases.
The percentage of $${P}_{2}{O}_{3}$$ in $${H}_{3}P{O}_{3}$$ is:
  • $$44.69$$
  • $$33.52$$
  • $$67.07$$
  • $$50.04$$
The total ionic strength of the solution containing $$0.1$$ M of $$CuS{O}_{4}$$ and $$0.1$$ M of $${Al}_{2}{(S{O}_{4})}_{3}$$ is :
  • 0.2 M
  • 0.19 M
  • 0.8 M
  • 0.105 M
In diammonium phosphate $$(NH_4)_2HPO_4$$, the percentage of $$P_2O_5$$ is :
  • 35.87
  • 46.44
  • 51.99
  • 53.78
Calculate the volume occupied by 40 g. of a $$CH_4$$ at S.T.P if its V.D. is 8. 
  • 24 litres
  • 46 litres
  • 34 litres
  • 56 litres
The volume occupied by 53.5 g of $$ Cl_2$$ is :
  • 15.76 litres
  • 16.87 litres
  • 18.65 litres
  • 20 litres
$$IE_{1}$$ for $$He$$ atom is 24.6 eV. The energy required to remove both the electrons from an atom in its ground state will be: 
  • 59 eV
  • 81 eV
  • 79 eV
  • None of these
Elements $$X, Y$$ and $$Z$$ have atomic numbers 5, 9 and 11 respectively. Which one forms an anion?
  • $$X$$
  • $$Y$$
  • $$Z$$
  • Both $$B$$ and $$C$$
A vessel contains N molecules of oxygen at a certain temperature and pressure. How many molecules of sulphur dioxide can the vessel accommodate at the same temperature and pressure.
  • N
  • 2N
  • N/2
  • 4N
Calculate the volume occupied by 0.01 moles of helium gas at STP.
  • 2.24 L
  • 0.224 L
  • 22.4 L
  • None of the above
The gases chlorine, nitrogen, ammonia and sulphur dioxide are collected under the same conditions of temperature and pressure. If 20 litres of nitrogen contains 'x' no. of molecules, state the no. of molecules in 20 litres of ammonia.
  • x
  • x/2
  • x/4
  • 2x
What is the volume occupied by X molecules of $$N_2$$?
  • 2V
  • 4V
  • V/2
  • V
An experiment was set up to determine the percentage of water absorbed by raisins. If the mass of dry raisins was $$40  g$$ and mass of wet raisins was $$45  g$$, the percent water absorbed would be:
  • $$\displaystyle\frac{45}{40}\times 100$$
  • $$\displaystyle\frac{40}{45}\times 100$$
  • $$\displaystyle\frac{45 - 40}{40}\times 100$$
  • $$\displaystyle\frac{45 - 40}{45}\times 100$$
A vessel contains X number of molecules of hydrogen gas at a certain temperature and pressure. Under the same conditions of temperature and pressure, how many molecules of nitrogen gas would be present in the same vessel?
  • 2X
  • X
  • 0.5X
  • 3X
Glucose is a physiological sugar. If the mass percentage of $$C=x\%$$, mass percent of $$H=y\%$$ and mass percent of $$O=z\%$$ in glucose $$(C_6H_{12}O_6)$$, then the value of $$x,\ y$$ and $$z$$ are, respectively:
  • $$40,\ 6.67,\ 53.33$$
  • $$30,\ 6.67,\ 43.33$$
  • $$40,\ 7.67,\ 63.33$$
  • none of the above
Insulin contains $$3.4$$% sulphur. The minimum molecular mass of insulin is :
  • $$940$$
  • $$350$$
  • $$470$$
  • $$560$$
If $$100$$ mL of $$H_2SO_4$$ and $$100$$ mL of $$H_2O$$ are mixed, the mass percent of $$H_2SO_4$$ in the resulting solution will be: 
$$(d_{H_2SO_4}=0.09\: g\: mL^{-1}, d_{H_2O}=1.0\: g\: mL^{-1})$$
  • $$90.32$$%
  • $$47.36$$%
  • $$50.56$$%
  • $$60$$%
The molar mass of hemoglobin is about $$65000 \: gmol^{-1}$$. Every hemoglobin contains $$4$$ iron atoms. Thus:
  • iron content in haemoglobin is $$0.35$$%.by mass
  • $$1$$ mole of haemoglobin contains $$56$$g iron
  • $$1$$ mole of haemoglobin contains $$224$$ g iron
  • if iron content is increased to $$0.56$$%, molar mass of hemoglobin would be higher than $$65000 \: g\: mol^{-1}$$
The molality of 1 L solution with x% $$H_2SO_4$$ is equal toThe weight of the solvent present in the solution is 910 g. The value of x in g per 100 mL is :
  • 90
  • 80.3
  • 40.13
  • 9
$$13.4$$ g of a sample of unstable hydrated salt, $$Na_2SO_4.xH_2O$$ was found to contain $$6.3$$ g of $$H_2O$$. The number of molecules of water of crystallisation is :
  • $$5$$
  • $$7$$
  • $$2$$
  • $$10$$
"Suvarnabhasm", an ayurvedic drug, is found to contain $$400$$ ppm of colloidal gold. Mass % of gold (atomic mass of Au $$=197$$ ) will be :
  • $$0.040\: %$$
  • $$7.88\: %$$
  • $$0.0788\: %$$
  • $$4\times 10^{-4}$$%
Four 1-1 litre flasks are separately filled with the gases $$H_2,\, He,\, O_2$$ and ozone. The ratio of total number of atoms of these gases present in different flask would be : 
  • 1 : 1 : 1 : 1
  • 1 : 2 : 2 : 3
  • 2 : 1 : 2 : 3
  • 3 : 2 : 2 : 1
A sample of $$H_{2}SO_{4}$$ contains $$3.2$$ kg of sulphur. The weight (in g) of hydrogen present in the sample is:
  • 100
  • 200
  • 50
  • 150
Statement: Equal volumes of all gases always contain equal number of moles.

State whether the given statement is true or false.
  • True
  • False
State True or False.
Mass of reactants is always equal to the mass of the products. (Don't consider nuclear reaction)
  • True
  • False
Law of conservation of mass was put forward by :
  • Lavoisier
  • Dalton
  • Priestly
  • Thomson
Two elements always combine together in a fixed ratio by weight.
  • True
  • False
State True or False.
Equal volumes of different gases under similar conditions of temperature and pressure contain equal number of atoms.
  • True
  • False
Atomic mass of an element is:
  • actual mass of one atom of the element
  • average mass of an atom of different atoms of the element
  • always a whole number
  • None of these
Under the same conditions, two gases have the same number of molecules. They must:
  • be noble gases
  • have equal volumes
  • have a volume of 22.4 dm$$^3$$ each
  • have an equal number of atoms
If $$1$$ L of $$O_2$$ at $$15^oC$$ and $$750$$ mm pressure contains $$\text N$$ molecules, the number of molecules in $$2$$ L of $$SO_2$$ under the same conditions of temperature and pressure will be :
  • $$\dfrac {\text N}{2}$$
  • $$\text N$$
  • $$2\text N$$
  • $$4\text N$$
Which of the following is the best thing to do during heavy lighting?
  • Lying on the ground in an open place
  • Going into the nearest water body
  • Staying indoors away from metallic doors or windows
  • Standing under a tall tree
The percentage value of nitrogen in urea is about :
  • $$46$$
  • $$85$$
  • $$18$$
  • $$28$$
3 g of a hydrocarbon on combustion in excess of oxygen produces 8.8 g of $$CO_2$$ and 5.4 g of $$H_2O$$. 

The data illustrates the law of :
  • Conservation of mass
  • Multiple proportions
  • Constant proportions
  • None of the above
The weights of two elements which combines with one another are in the ratio of their:
  • atomic weight
  • molecular weight
  • equivalent weight
  • none of the above
Modern atomic mass scale is based on the mass of:
  • $$H - 1$$
  • $$C - 12$$
  • $$C - 14$$
  • $$C - 16$$
Insulin contains $$3.4$$% sulphur. The minimum molecular weight of insulin is :
  • 941.176
  • 944
  • 945.27
  • none
Photo-electric cell is not used in:
  • television
  • photography
  • reproduction of sound in cinema
  • automatic switching of street lightening circuits
Percentage of Se in peroxidase anhydrous enzyme is $$0.5$$% by weight (At. wt. = $$78.4$$) then, minimum molecular weight of peroxidase anhydrous enzymes is :
  • $$\displaystyle 1.568\times 10^{4}$$
  • $$\displaystyle 1.568\times 10^{3}$$
  • $$15.68$$
  • $$\displaystyle 2.136\times 10^{4}$$
The density of a salt solution is $$1.13 g cm^{-3}$$ and it contains $$18\%$$ of $$NaCI$$ by weight The volume of the solution containing $$36.0\ g$$ of the salt will be
  • $$200 cm^3$$
  • $$217 cm^3$$
  • $$177 cm^3$$
  • $$157 cm^3$$
$$10\ g$$ of a crystalline metal sulphate salt when heated generates approximately $$6.4\ g$$ of an anhydrous salt of the same metal. The molecular weight of the anhydrous salt is $$160\ g$$. The number of water molecules present in the crystal is
  • $$1$$
  • $$2$$
  • $$3$$
  • $$5$$
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Practice Class 11 Medical Chemistry Quiz Questions and Answers