Calculate the volume, mass and number of molecules of hydrogen liberated when 230 g of sodium reacts with excess of water at STP (atomic masses of Na = 23U, O = 16 U and H = 1U).

Calculate the volume, mass and number of molecules of hydrogen liberated when 230 g of sodium reacts with excess of water at STP. (atomic masses of Na = 23U, O = 16U, and H = 1U) the balanced equation for the above reaction is {:(2Na_((s))+2H_(2)O_((l)),,to2NaOH_((aq)) +H_(2(g))+H_(2(g))uparrow),((2xx23)U+ 2(2xx1 +1 xx 16)U,,to2(23+16+1)U+(2xx1)U),(46 U + 36U,,to80U + 2U),(or46g + 36g ,, to 80 g + 2 g):}

The molecular mass of sulphuric acid is (Atomic masses of S = 32, O=16 and H=1)-

Molecular mass of HNO_3 (Atomic masses of H=1U, N=14U, O=16U)-

The weight of iodine liberated when excess of KI reacts with 500 ml of 1 M H_2O_2 is

Calculate the volume of CO_(2) obtained at STP when 2.12 g of Na_(2)CO_(3) reacts with excess of dil HCI .

write the question for reaction of zinc with hydrochloric acid and balance the equation find out the number of molecules of hydrogen gas produced in this reaction, when 5 mole of HCL completely reacts at STP (Gram molar volume is 22.4 litres at STP, Avogadro’snumber is 6.023 xx 10^(23)

How many litres of _2 at STP will be formed when 100 ml of 0.1 M, H_2S)_4 reacts with excess of Na_2CO_3 ?

What is the volume of oxygen liberated at S.T.P When 3.4g of H_(2)O_(2) is heated?

On the basis of the postulates of kinetic theory of gases, it is possible to derive the mathematical expression, commonly known as kinetic gas equation. PV = 1/3 m n u^3? where, P= Pressure of the gas, V a volume of the gas, m=Mass of a molecule, n = Number of molecules present in the given amount of a gas and u = root mean square speed For one mole of gas, PV = RT and n=N_A 1/3 m N_a u^2 = RT or 2/3 .1/2m N_A u^2 = N_A [1/2mN_Au^2 = KE "per mole"] ,2/3K.E. = RT implies K.E. 3/2RT Average kinetic energy per mol does not depend on the nature of the gas but depends only on temperature. This, when two gases are mixed at the same temperature, there will be no rise or decrease in temperature unless both react chemically. Average kinetic energy per molecule = ("Average K.E. per mole")/N = 3/2(RT)/(N) implies 3/2kT where k is the Boltzmann constant The average kinetic energy (in joule) of the molecules in 8g methane at 27&@C is.