Fill in the blanks. a) In a chemical r...

Fill in the blanks.
a) In a chemical reaction, the sum of the masses of the reactants and products remains unchanged. This is called law of conservation of mass.
b) A groupof atoms carrying a fixed charge on them is called polyatomic ion.
The formula unit masss of `Ca_(3)(PO_(4))_(2)` is 310g.
d) Formula of sodium carbonate is .............. and that of ammonium sulphate is.............

Text Solution

Verified by Experts

(a)Law of conservation of mass
(b)Polyatomic ions
(c )`3xx"Atomic mass of Ca"+2xx"Atomic mass of P"+8xx"Atomic mass of O"`
`=3xx40+2xx31+8xx16=120+62+128=310u`
(d)`Na_(2)CO_(3), (NH_(4))_(2)SO_(4)`

Topper's Solved these Questions

ATOMS AND MOLECULES
DINESH PUBLICATION|Exercise SHORT ANSWER QUESTIONS|13 Videos
IS MATTER AROUND US PURE
DINESH PUBLICATION|Exercise LAQs|10 Videos

Similar Questions

Explore conceptually related problems

Fill in the following blanks with suitable words : (a) In water , the proportion of oxygen and hydrogen is "…………." by mass. (b) In a chemical reaction, the sum of the masses of reactants and the products remains unchanged. This is called "..........." .

In a chemical reaction, 10.6g of sodium carbonate reacted with 12g of ethanoic acid. The products obtained were 4.4g of carbon dioxide, 16.4 of sodium ethanoate and 1.8g of water. (a)Write a word equation, clearly showing the reactants and products as given above. (b)Also show that this data is in aggrement with the law of conservations of mass.

Fill in the following blanks with suitable words: (a) The form of carbon which is know as black lead is …….. (b) The form of carbon which is used as a lubricant at high temperature is….. (c ) compounds of carbon with hydrogen alone are called ....... (d) C_(n)H_(2n) is the general foumula of .................... hydrocarbons. (e ) Hydrocarbons haveing the general formula C_(n)H_(2n-2) are called ................... (f) Ethyne and ethyne are examples of ....................hydrocatbons. (g) Ethyne has .................. carbon hydrogen single bonds. (h) carbon compounds have usually ................. melting p[oints and boiling points beacuse they are.................. in nature. (i) The prperty of carbon atoms to form along chains in compounds is called........... (J) The general formaula C_(n)H_(2n) for cycloalkanes is the same as that of ................ (k) The IUPAC name of ethylene is .................... (l) The IUPAC name of acetyleneis ........................

Ravi was performing some experiements related to the laws of chemical combination in the science laboratory under the guidance of his chemistry teacher Mr. John. Ravi found that when he burned 1 gram of hydrogen gas in 8 grams of oxygen gas in a closed vessel, he obtained 9 grams of water. He repeated this experiment many times but obtained the same results every time (a) Write a balanced chemical equation for the reaction between hydrogen and oxygen to form water. Also write the names of all the substances involved below their formulae in the equation (b) What are the reactants and products in the above reaction ? (c) Which law of chemical combination is illustrated by the fact that when Ravi burned 1g of hydrogen in 8g of oxygen, he obtained 9g of water ? (d) What mass of water will be obtained if 1g of hydrogen is burned in 10g of oxygen ? Which law of chemical combination will govern your answer ? (e) What values are displayed by Ravi in this episode ?

Fil in the blanks a. The mass of 1 molecule of water (H_(2) O) is ……… b. The number of molecules in 16 g of sulphur dioxide (SO_(2)) are ………. c. The weight of one mole of sodium carbonate (Na_(2) CO_(3)) is…………….. d. Moles and g equivalent in 196 g of Ca (OH)_(2) are ...... and ....... e. Moles and g equivalent in 196 g of H_(3) PO_(4) are ............. and ............ f. g atoms in 62 g of P_(4) are ....... f. g atoms in 24 g of magnesium are...........

Equivalent Mass The eqivalent mass of a substance is defined as the number of parts by mass of it which combine with or displace 1.0078 parts by mass of hydrogen, 8 parts by mass of oxygen and 35.5 parts by mass of chlorine. The equivalent mass of a substance expressed in grams is called gram equivalent mass. The equivalent mass of a substance is not constant. It depends upon the reaction in which the substance is participating. A compound may have different equivalent mass in different chemical reactions and under different experimental conditions. (a) Equivalent mass of an acid It is the mass of an acid in grams which contains 1.0078 g of replaceable H^(+) ions or it is mass of acid which contains one mole of replaceable H^(+) ions. It may be calculated as : Equivalent mass of acid= ("Molecular mass of acid")/("Basicityof acid ") Basicity of acid = Number of replaceable hydrogen atoms present in one molecule of acid (b) Equivalent mass of a base It is the mass of the base which contains one mole of replaceable OH^(-) ions in molecules. Equivalent mass of base= ("Molecular mass of acid ")/("Acidity of acid") Acidity of base= Number of replaceable OH^(-) ions present in one molecule of the base Equivalent mass of an oxidising agent (a) Electron concept: Equivalent mass of oxidising agent = ("Molecular mass of oxidising agent")/("Number of electrons gained by one molecule") (b) Oxidation number concept: Equivalent mass of oxidising agent= ("Molecular mass of oxidising agent")/("Total change in oxidation number per molecule of oxidising agent") Equivalent weight of oxalic acid salt in following reaction is :( Atomic masses:O=16,C=12,K=39) H_(2)C_(2)O_(4)+Ca(OH)_(2) toCaC_(2)O_(4)+H_(2)O

Equivalent Mass The eqivalent mass of a substance is defined as the number of parts by mass of it which combine with or displace 1.0078 parts by mass of hydrogen, 8 parts by mass of oxygen and 35.5 parts by mass of chlorine. The equivalent mass of a substance expressed in grams is called gram equivalent mass. The equivalent mass of a substance is not constant. It depends upon the reaction in which the substance is participating. A compound may have different equivalent mass in different chemical reactions and under different experimental conditions. (a) Equivalent mass of an acid It is the mass of an acid in grams which contains 1.0078 g of replaceable H^(+) ions or it is mass of acid which contains one mole of replaceable H^(+) ions. It may be calculated as : Equivalent mass of acid= ("Molecular mass of acid")/("Basicityof acid ") Basicity of acid = Number of replaceable hydrogen atoms present in one molecule of acid (b) Equivalent mass of a base It is the mass of the base which contains one mole of replaceable OH^(-) ions in molecules. Equivalent mass of base= ("Molecular mass of acid ")/("Acidity of acid") Acidity of base= Number of replaceable OH^(-) ions present in one molecule of the base Equivalent mass of an oxidising agent (a) Electron concept: Equivalent mass of oxidising agent = ("Molecular mass of oxidising agent")/("Number of electrons gained by one molecule") (b) Oxidation number concept: Equivalent mass of oxidising agent= ("Molecular mass of oxidising agent")/("Total change in oxidation number per molecule of oxidising agent") When NO_(2) is dissolved in water solution become acidic. Equivalent weight of NO_(2) in this reaction (NO_(2)+H_(2)O to HNO_(3)+HNO_(2)) is :

Equivalent Mass The eqivalent mass of a substance is defined as the number of parts by mass of it which combine with or displace 1.0078 parts by mass of hydrogen, 8 parts by mass of oxygen and 35.5 parts by mass of chlorine. The equivalent mass of a substance expressed in grams is called gram equivalent mass. The equivalent mass of a substance is not constant. It depends upon the reaction in which the substance is participating. A compound may have different equivalent mass in different chemical reactions and under different experimental conditions. (a) Equivalent mass of an acid It is the mass of an acid in grams which contains 1.0078 g of replaceable H^(+) ions or it is mass of acid which contains one mole of replaceable H^(+) ions. It may be calculated as : Equivalent mass of acid= ("Molecular mass of acid")/("Basicityof acid ") Basicity of acid = Number of replaceable hydrogen atoms present in one molecule of acid (b) Equivalent mass of a base It is the mass of the base which contains one mole of replaceable OH^(-) ions in molecules. Equivalent mass of base= ("Molecular mass of acid ")/("Acidity of acid") Acidity of base= Number of replaceable OH^(-) ions present in one molecule of the base Equivalent mass of an oxidising agent (a) Electron concept: Equivalent mass of oxidising agent = ("Molecular mass of oxidising agent")/("Number of electrons gained by one molecule") (b) Oxidation number concept: Equivalent mass of oxidising agent= ("Molecular mass of oxidising agent")/("Total change in oxidation number per molecule of oxidising agent") Equivalent mass of Ba(MnO_(4))_(2) in acidic medium is :(where M stands for molar mass)

The number of carbon atoms in exactly 12 g C^(12) is called Avogadro's number , N_(A) (6.022 xx 10^(23)) . One mole is the amount of material which contains Avogradro's number of particle. These definitions emphasize that the mole refers to a fixed number of NA^(+) b Avogadro's number of atoms , electrons to refer to a mole of helium , a mole of electrons , or a mole of NA^(+) by Avogadro's number of atoms, electrons or ions respectively. On the other hand, phrases like "one mole of hydrogen" can be ambiguous , and should be restated as "one mole of hydroden atoms" or " one mole fo hydrogen molecules." But it is a matter of common practice among chemists , however , to let the name of the element stand for its mos common form. Thus one mole of O_(2) is frequently referred to as one mole of oxygen , whereas one moles of O is called one mole of oxygen atoms. Suppose if we take one mole molecules fo H_(2)SO_(4) then it contain 2 moles of H atom 1 mole of S atom and 4 moles of O atom. It can also be said that moles of oxygen molecules is (4)/(2) =2 mole. From a mixture of 4 moles Ca_(3)(PO_(4))_(2) , 5 moles of p_(4)O_(10) and 6 moles of H_(3)PO_(3) , all the phosphourus atoms are removed . Then moles of P_(4) molecules formed from all these atoms are:

The number of carbon atoms in exactly 12 g C^(12) is called Avogadro's number , N_(A) (6.022 xx 10^(23)) . One mole is the amount of material which contains Avogradro's number of particle. These definitions emphasize that the mole refers to a fixed number of NA^(+) b Avogadro's number of atoms , electrons to refer to a mole of helium , a mole of electrons , or a mole of NA^(+) by Avogadro's number of atoms, electrons or ions respectively. On the other hand, phrases like "one mole of hydrogen" can be ambiguous , and should be restated as "one mole of hydroden atoms" or " one mole fo hydrogen molecules." But it is a matter of common practice among chemists , however , to let the name of the element stand for its mos common form. Thus one mole of O_(2) is frequently referred to as one mole of oxygen , whereas one moles of O is called one mole of oxygen atoms. Suppose if we take one mole molecules fo H_(2)SO_(4) then it contain 2 moles of H atom 1 mole of S atom and 4 moles of O atom. It can also be said that moles of oxygen molecules is (4)/(2) =2 mole. According to common practise , if you have Avogadro number of hydrogen molecules, then its mass is equal to :

DINESH PUBLICATION-ATOMS AND MOLECULES-LONG ANSWER QUESTIONS

Cinnabar (HgS) is a prominent ore of mercury. How many grams of mercur...
Text Solution
|
The mass of one steel screw is 4.11 g. Find the mass of the of one mol...
Text Solution
|
A sample of vitamin C is known to contain 2.58 xx 10^(24) oxygen atoms...
Text Solution
|
Raunak took 5 moles of carbon atoms in a container and Krish also took...
Text Solution
|
Fill in the missing data in the given table
Text Solution
|
The visible universe is estimated to contain 10^(22) stars. How many m...
Text Solution
|
What is the SI prefix for each of the following multiples and submulti...
Text Solution
|
Express each of the following in kilograms a) 5.84 xx 10^(-3)mg b)...
Text Solution
|
Compute the difference in masses of 10^(3) moles of each of magnesium ...
Text Solution
|
Which has more number of atoms? 100g of N(2) or 100g of NH(3)
Text Solution
|
Compute the number of ions present in 5.85g of sodium chloride.
Text Solution
|
A gold sample contains 90% of gold and the rest copper. How many atoms...
Text Solution
|
What are ionic and molecular compounds? Give exmples.
Text Solution
|
Compute the difference in masses of one mole each of aluminium atoms a...
Text Solution
|
A silver ornament of mass 'm' gram is polished with gold equivalent to...
Text Solution
|
A sample of ethane (C(2)H(6)) gas has the same mass a 1.5 xx 10^(20) m...
Text Solution
|
Fill in the blanks. a) In a chemical reaction, the sum of the masses...
Text Solution
|
Complete the followiing crossword puzzle by using the nameof the chemi...
Text Solution
|
Write the formulae for the following and calculate the molecular mass ...
Text Solution
|
In photosynthesis, 6 molecules of carbon combine with an equal number ...
Text Solution
|