(C) The mass of hydrogen in a $75 \ kg$ human body is calculated as: $\text{Mass of } H = \frac{10}{100} \times 75 \ kg = 7.5 \ kg$. When all $^1H$ at

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(C) The mass of hydrogen in a $75 \ kg$ human body is calculated as: $\text{Mass of } H = \frac{10}{100} \times 75 \ kg = 7.5 \ kg$. When all $^1H$ atoms (atomic mass $\approx 1$) are replaced by $^2H$ atoms (atomic mass $\approx 2$),the mass of the hydrogen component doubles. New mass of hydrogen $= 7.5 \ kg \times 2 = 15 \ kg$. Therefore,the weight gain is $15 \ kg - 7.5 \ kg = 7.5 \ kg$.

Class 11 Chemistry Some Basic Concepts of Chemistry Chemical stoichiometry

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The most abundant elements by mass in the body of a healthy human adult are: Oxygen $(61.4\%);$ Carbon $(22.9\%),$ Hydrogen $(10.0\%);$ and Nitrogen $(2.6\%).$ The weight which a $75 \ kg$ person would gain if all $^1H$ atoms are replaced by $^2H$ atoms is ....... $kg$.

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A
$15$
B
$37.5$
C
$7.5$
D
$10$

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Some Basic Concepts of Chemistry

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Chemical stoichiometry

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How many moles of $H_2O$ are liberated when one mole of hydrated $MgCl_2$ is heated?

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One litre of hard water contains $12.00 \ mg$ of $Mg^{2+}$. The milli-equivalents of washing soda $(Na_2CO_3)$ required to remove its hardness is:

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$A$ solution of $CaCl_2$ is $0.5 \, mol/L$. The number of moles of chloride ions in $500 \, mL$ of this solution will be:

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Complete combustion of $3 \ g$ of ethane gives $x \times 10^{22}$ molecules of water. The value of $x$ is ......... (Round off to the Nearest Integer). [Use: $N_{A} = 6.023 \times 10^{23} ;$ Atomic masses in $u$ $C = 12.0, O = 16.0, H = 1.0$]

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What will be the amount of $MgCl_2$ produced when $17 \ g$ of $HCl$ is reacted with an excess of $MgO$ in the following reaction?
$MgO + 2HCl \longrightarrow MgCl_2 + H_2O$

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The most abundant elements by mass in the body of a healthy human adult are: Oxygen $(61.4\%);$ Carbon $(22.9\%),$ Hydrogen $(10.0\%);$ and Nitrogen $(2.6\%).$ The weight which a $75 \ kg$ person would gain if all $^1H$ atoms are replaced by $^2H$ atoms is ....... $kg$.

Similar Questions

How many moles of $H_2O$ are liberated when one mole of hydrated $MgCl_2$ is heated?

One litre of hard water contains $12.00 \ mg$ of $Mg^{2+}$. The milli-equivalents of washing soda $(Na_2CO_3)$ required to remove its hardness is:

$A$ solution of $CaCl_2$ is $0.5 \, mol/L$. The number of moles of chloride ions in $500 \, mL$ of this solution will be:

Complete combustion of $3 \ g$ of ethane gives $x \times 10^{22}$ molecules of water. The value of $x$ is ......... (Round off to the Nearest Integer). [Use: $N_{A} = 6.023 \times 10^{23} ;$ Atomic masses in $u$ $C = 12.0, O = 16.0, H = 1.0$]

What will be the amount of $MgCl_2$ produced when $17 \ g$ of $HCl$ is reacted with an excess of $MgO$ in the following reaction? $MgO + 2HCl \longrightarrow MgCl_2 + H_2O$

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What will be the amount of $MgCl_2$ produced when $17 \ g$ of $HCl$ is reacted with an excess of $MgO$ in the following reaction?
$MgO + 2HCl \longrightarrow MgCl_2 + H_2O$