Suppose the elements X and Y combine to form two compounds \ce{XY2} and \ce{X3Y2}. When 0.1 mole of \ce{XY2} weighs 10 g and 0.05 mole of \ce{X3Y2} weighs 9 g, the atomic weights of X and Y respectively are
Which of the following concentration terms is dependent on temperature?
A mixture of 2.3 g formic acid (\ce{HCOOH}) and 4.5 g oxalic acid (\ce{(COOH)2}) is treated with conc. \ce{H2SO4}. The evolved gaseous mixture is passed through \ce{KOH} pellets. The weight (in g) of the remaining gas is
In which of the following is the number of water molecules maximum?
The number of moles of hydrogen molecules required to produce 20 moles of ammonia through the Haber process is
The density of a 2 M aqueous solution of \ce{NaOH} is 1.28 g cm$^{-3}$. The molality of the solution is (molar mass of \ce{NaOH} = 40 g mol$^{-1}$)
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Which one of the following has the maximum number of atoms?
An organic compound contains 78\% (by wt.) carbon and the remaining percentage of hydrogen. The empirical formula of the compound is [at. wt.: C = 12, H = 1]
What mass of 95\% pure \ce{CaCO3} is required to neutralise 50 mL of 0.5 M \ce{HCl} according to the reaction below? (answer to second decimal place) \ce{CaCO3(s) + 2HCl(aq) -> CaCl2(aq) + CO2(g) + 2H2O(l)}
In a one molal solution that contains 0.5 mole of a solute, there is
The weight (g) of two moles of the organic compound obtained by heating sodium ethanoate with sodium hydroxide in the presence of calcium oxide is
The mass of \ce{CO2} produced by heating 20 g of 20\% pure limestone is (at. mass Ca = 40) \ce{CaCO3 ->[1200 K] CaO + CO2}
The density of a 1 M solution of a compound X is 1.25 g mL$^{-1}$. The molality of the solution is (molar mass of X = 85 g mol$^{-1}$)
The highest number of helium atoms is present in
1 gram of \ce{NaOH} is treated with 25 mL of 0.75 M \ce{HCl} solution. The mass of \ce{NaOH} left unreacted is
A compound X contains 32\% of A, 20\% of B and the remaining percentage of C. The empirical formula of X is (atomic masses: A = 64, B = 40, C = 32 u)
Among the following, choose the ones with an equal number of atoms. A. 212 g of \ce{Na2CO3}(s) [molar mass = 106 g] B. 248 g of \ce{Na2O}(s) [molar mass = 62 g] C. 240 g of \ce{NaOH}(s) [molar mass = 40 g] D. 12 g of \ce{H2}(g) [molar mass = 2 g] E. 220 g of \ce{CO2}(g) [molar mass = 44 g] Choose the correct answer from the options given below:
Dalton's atomic theory could \emph{not} explain which of the following?
The numbers $17.0145$ and $21.0235$ were rounded to three figures after the decimal point. The resulting numbers, respectively, are:
The number of hydrogen atoms present in 5.4 g of urea is (molar mass of urea = 60 g mol$^{-1}$; $N_A = 6.022\times10^{23}$ mol$^{-1}$)
When 1 dm$^3$ of \ce{CO2} gas is passed over hot coke, the volume of the gaseous mixture after complete reaction at STP becomes 1.4 dm$^3$. The composition of the gaseous mixture at STP is
The amount of carbon dioxide evolved upon complete combustion of $116\,$g of n-butane is: (Atomic masses: H $=1$, C $=12$, O $=16$)
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