56g of `N_(2)` reacts with 9g of `H_(2)` in a closed vessel to form `NH_(3)`. Which reactant is left in excess and how much

1.0 g of magnesium is burnt with 0.56 g O_2 in a closed vessel. Which reactant is left in excess and how much? (At.wt: Mg=24, O = 16)

1g of Mg is burnt in a closed vessel which contains 0.5g of O_(2) (i) Which reactants is left in excess (ii) Find the mass of the excess reactant.

3.00 g of H_(2) react with 28.00 g of O_(2) to yield H_(2)O . Which is the limiting reactant ?

B_(2)H_(6) reacts with NH_(3) to form

B_(2)H_(6) reacts with NH_(3) to form

6 g of H_(2) reacts with 14 g N_(2) to form NH_(3) till the reaction completely consumes the limiting reagent. The mass of other reactant (in g) left are ……

2 mol of N_(2) is mixed with 6 mol of H_(2) in a closed vessel of one litre capacity. If 50% N_(2) is converted into NH_(3) at equilibrium, the value of K_(c) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)

10 ml N_(2) is reacted with 20 ml H_(2) to form NH_(3) . The correct statements is /are

3.00 g of H_(2) react with 28.00 g of O_(2) to yield H_(2)O . Calculate the mass of one of the reactants which remains unreacted.

Calculate the work done when 56g of iron reacts with hydrochloric acid in (a) a closed vessel of fixed volume and (b) an open beaker at 25^(@)C .