one litre of a certain gas weighs 2 g at 300 k and 1 atm pressure. if pressure is reduced to 0.75 atm, then at which temperature 1 litre of the gas will weigh equal to 1 gm
450 k
recall: dalton’s law of partial pressures states that the total pressure of a mixture of unreacting gases is the sum of the partial pressures of the individual gases.the partial pressure of a gas in the mixture is the product of the total pressure of the mixture and the mole fraction, χ, of the gas:we first need to calculate the mole fraction of the gases before calculating their partial pressures. the molar mass of o2 is 2(16.00 g/mol o) = 32.00 g/mol and the molar mass of co2 is 12.01 g/mol c + 2(16.00 g/mol o) = 44.01 g/mol.[readmore]the moles of o2 and co2 in the tank are:the total moles of gas is 1.6406 mol + 1.4792 mol = 3.1198 mol.the mole fraction of o2 and co2 are:the total pressure in the tank is 9.21 atm. the partial pressures of o2 and co2 are: 1.5 kg = 1.5 × 1000 g = 1500 g∴ ratio of 1.5 kg to 2500 g= 1500 g : 2500 g = `1500/2500` = `3/5` = 3 : 5 radius = 1.75 m
height (h) = 12 m
volume = 
= ×  × 1.75 × 1.75 × 12
= 38.5 m3
since, 1 m3 = 1 kiloliter
capacity of the pit = (38.5 × 1)
= 38.5 kilolitres one pascal is defined as the 1 newton force applied on an area of 1 m2. it is the si unit of pressure. also 1 pa = 1 kg. [readmore]typed answera) δg° = -rtlnksp δg° = -(8.314 jmol-k)(298k)ln(4.6×10-2 )= 7628.72 j = 7.63 kjb) ∆g° = nfe°e° = ∆g°-nfe° = 7.63-(2)(96,000)(11000)e° =-0.0397 v mass (molar mass) → mol (avogadro's number) → molecules[readmore]3.51×104 g ×1 mol163.94 g×6.022×1023 molecules1 mol = 1.29x1026 moleculesthere are 1.29x1026 molecules in the sample your cubic meter box contains about 1.2 kg of air. the specific heat of air is about 1 kilojoule per kilogram per degree centigrade.

so 1.2 kilojoules per degree centigrade. to get from 20c to 1000c you need 980 * 1.2 = 1176 kilojoules = 327 watt-hours. you can get 1440 watts from a us 15a hous… for water, h2o1 mol h2o = 18.0 g h2o1 mole h2o = 6.022x1023 h2o molecules[readmore]the number of h2o molecules in a 9.00-g sample of water:9.00 g h2o×1 mol h2o18.0 g h2o×6.022×1023 h2o molecules1 mol h2o= 3.01x1023 h2o moleculesthe number of h2o molecules in a 9.00-g sample of water is 3.01x1023 h2o molecules. answer: the molecular mass of an element is defined as the sum of the masses of the elements present in the molecule. molecular mass is obtained by multiplying the atomic mass of an element with the number of atoms in the molecule and then adding the masses of all the elements in the molecule. o2 is a diatomic molecule. the mass of an oxygen atom = 16 amu. ∴ mass of o2 molecule = 2 × 16 = 32 amu. mass of one molecule of oxygen → 32/ avogadro constant ( 6.023 × 1023) → 5.31 × 10-23g. kclo3(s) — heat→ kcl (s) + o2(g)      reactant        productk        1                   1cl       1                   1o       3                    2[readmore]2 kclo3(s) — heat→ 2 kcl (s) + 3 o2(g)      reactant        productk        2                   2cl       2                   2o       6                    6the balanced equation for the reaction is 2 kclo3(s) — heat→ 2 kcl (s) + 3 o2(g)