The mass of `N_2F_4` produced by the reaction of `2.0g` of `NH_3 and 8.0g` of `F_2` is `3.56g`. What is the per cent yield ?

The mass of N_(2)F_(4) produced by the reaction of 2.0 g of NH_(3) and 8.0 g F_(2) is 3.56 g. What is the per cent yield ?

What mass of P_(4) O_(10) will be produced by the combustion of 2.0 g of P_(4) with 2.0 g of O_(2)

What volume of H_(2)(g) is produced by decomposition of 2.4 L NH_(3) (g) ? .

What per cent of 2 kg is 125 g ?

For the reaction, N_2[g] + 3H_2[g] hArr 2NH_3[g] , Delta H = …

0.6 mole of NH_(3) in a reaction vessel of 2dm^(3) capacity was brought to equilibrium. The vessel was then found to contain 0.15 mole of H_(2) formed by the reaction 2NH_(3)(g) hArr N_(2)(g)+3H_(2)(g) . Which of the following statements is true?

In the reaction, N_2(g) +3H_2(g) hArr 2NH_3(g) the value of the equilibrium constant depends on

For the reaction N_(2)(g) + 3H_(2)(g) rarr 2NH_(2)(g) Which of the following is correct?

Conisder the chemical reaction N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g) The rate of this reaction can be expressed in terms of time derivatives of the concentration of N_(2)(g), H_(2)(g) , or NH_(3)(g) . Identify the correct relationship among the rate expresisons.

A mixture of 2 moles of N_2,2.0 moles of H_2 and 10.0 moles of NH_3 is introduced into a 20.0 L reaction vessel at 500 K . At this temperature, equilibrium constant K_c is 1.7 xx 10^2 , for the reaction N_2(g) +3H_2(g) hArr 2NH_3(g) (i) is the reaction mixture at equilibrium ? (ii) if not, what is the direction of the reaction ?