What is the mass of precipitate formed when 50 ml of 8.5 % solution of AgNO₃ is mixed with 100 ml of 1.865 % potassium chloride solution ?

Which among the following statement(s) describe an element?
i) It is a pure substance which could be split into two or more simpler substance.
ii) It is a pure substance which cannot be split into simpler substance
iii) It's composition is not uniform
iv) All the above

How many moles of magnesium phosphate Mg₃(PO₄)₂ Will Contain 0.25 moles of oxygen atoms?

Assertion: Equal volumes of all the gases do not contain equal number of atoms
Reason: Atom is the smallest particle which takes part in chemical reactions.
Codes:
(a) Both assertion and reason are correct and reason is the correct explantion for assertion
(b) Both assertion and reason are correct but reason  is not the correct explantion for assertion
(c) Assertion is true but reason are false
(d) Both assertion and reason are false

Two elements X and Y ( atomic mass of X = 75; Y = 16) combine to give a compound having 76% of X. The formula of the compound is?

The percentage yield of reaction can be described as the.................................times 100%.

How many significant figures should be used for the answer to the following calculation?

\(\frac { (0.82056)\ (298.15)\ (0.379) }{ (0.9480) } \)

In the reaction, 4NH₃(Xg) + 5O₂(g) \(\rightarrow \) 4NO(g)+6H₂O(I) when 1 mole of ammonia and mol of O₂ are made to reactent completion then

In the reaction of sodium thiosulphate with I₂ in aqueous medium, the equivalent weight of dodium thisulphate is equal to

The number of moles of H₂ in 0.224 L of hydrogen gas at STP (273 K, 1 atm) is

The molarity of water given its density is 1000 kg m^-3  is

The number of molecules in 16g of methane is _________

How many equivalents of sodium sulphate is formed when sulphuric acid is completely neutralized by a base NaOH __________.

How many molecules of hydrogen is required to produce 4 moles of ammonia?

The number of moles of H, in 2.24 litre of hydrogen gas at STP is ____________

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.

What is the empirical formula of the following?
i) Fructose (C₆ H₁₂ O₆) Found in honey
ii) Caffeine  (C₈ H₁₀ N₄ O₂) a substance found in tea and Coffee 

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) 
iii) 
iv) 

Calculate the equivalent masses of the following - HNO₃

What is meant by Plasma state? Give an example.

Calculate the mass of the following : 1 atom of silver

How much mass (in gram units) is represented by the following ?
0.2 mol of NH₃

Calculate the oxidation number of underlined atoms of the following :
NO₃^-

Calculate the number of moles present in the following 120g of sodium hydroxide

Define the following:
(i) Element
(ii) Compound.

Balance the following equations by oxidation number method.
K₂Cr₂O₇ + HI ⟶ KI + Crl₃ + H₂O + I₂

\({ 2NH }_{ 3 }\left( g \right) +{ CO }_{ 2 }\left( g \right) \rightarrow \underset{Urea}{H_2N}-\overset { \underset { || }{ O } }{ C } -{ NH }_{ 2 }\left( aq \right) +{ H }_{ 2 }O(I)\)
In a process, 646 g of ammonia is allowed to react with 1.144 kg of CO₂ to form urea.
(i) If the entire quantity of all the reactants is not consumed in the reaction which is the limiting reagent ?
(ii) Calculate the quantity of urea formed and unreacted quantity of the excess reagent. The balanced equation is 
\(\overset { { 2NH }_{ 3 }+{ CO }_{ 2 } }{ \underset { { H }_{ 2 }NCON{ H }_{ 2 }+{ H }_{ 2 }O }{ \downarrow } } \)