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_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_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 ?

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

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 .

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?

In the reaction 2NH_(3)(g)+5F_(2) to N_(2)F_(4)+6HF 3.56g N_(2)F_(4) is obatained by mixing 2g NH_(3) and 8g F_(2) . The percentage yield of the production is:

In Haber's process 50.0 g of N_(2)(g) and 10.0 g of H_(2)(g) are mixed to produce NH_(3)(g) . What is the number of moles of NH_(3)(g) formed?