The mass of `N_2F_2` 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_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 ?

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 ?

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 ?

Ammonia is produced in accordance with this equation . N_(2)(g) + 3H_(2)(g) rightarrow 2NH_(3)(g) In a particular experiment, 0.25mol of NH_(3) is formed when 0.5 mol of N_(2) is reacted with 0.5 mol of H_(2) . What is the percent yield?

What mass of N_2 will be required to produce 34 g of NH_3 by the reaction , N_2+3H_2 to 2NH_3 .

For the reaction : 2 NH_(3)(g) rarr N_(2)(g) + 3 H_(2)(g)

For the reaction, N_(2)(g)+3H_(2)(g) to 2NH_(3)(g)