Analyse the following equation `2NO_((g))+O_(2(g))rarr2NO_(2(g))`: Calculate the mass of `NO_2` formed when 112L of oxygen react completely?

Analyse the following equation 2NO_((g))+O_(2(g))rarr2NO_(2(g)) : Calculate the number of the moles of NO required to combine completely with 112L of Oxygen at STP.

The balanced chemical equation of a reaction (at STP) is given below. 2H_(2((g))+O_(2(g))rarr2H_2O_((g)) : Calculate the mass of water formed as a result of the reaction (a).

Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical equation: 'N_2(g)+3H_2(g) rarr 2NH_3(g)' i. Calculate the mass of ammonia produced if '2.00 xx 10^3' g dinitrogen reacts with '1.00 xx 10^3 g of dihydrogen. ii. Will any of the two reactants remain unreacted? iii. If yes, which one and what would be its mass?

The balanced chemical equation of a reaction (at STP) is given below. 2H_(2((g))+O_(2(g))rarr2H_2O_((g)) : Calculation the volume of oxygen required to combine completely with 224L of the hydrogen at STP.

If 6.023xx10^23 molecules of N_2 react completely with H_2 according to the equation: N_(2(g)) + 3H_(2(g)) rarr 2NH_(3(g)) , then calculate the numbers of molecules of NH_3 formed.

Look at the balance equation given. 2NaOH+CO_2rarrNa_2CO_3+H_2O : Find out the mass of NaOH needed for 264 g CO_2 to react completely.

The CHEical equation for the manufacture of ammonia is N_2(g)+3H_2(g) to 2NH_3(g) Calculate the amount of H_2 required to react with 28 g of N_2 , completely. [Hint Molecular mass of N_2 = 28 , H_2 =2 ]

For the reaction, 2NO_((g) + O_(2(g) rarr 2NO_(2(g) the rate law is given as. Rate =k [NO]^2[O_2] The order of the reaction with respect to O_2 is _______

Calculate the amount of CO_2 produced when 2 moles of carbon are burned in l6 g of O_2