Amount of NO(g) formed by oxidation of 1 mole of `NH_(3)(g)` using 1 mole of `O_(2)(g)`is (A) 4.8 g (B) 56.0g (C) 30.0g (D) 24.0g

One mole of N_(2) (g) is mixed with 2 moles of H_(2)(g) in a 4 litre vessel If 50% of N_(2) (g) is converted to NH_(3) (g) by the following reaction : N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) What will the value of K_(c) for the following equilibrium ? NH_(3)(g)hArr(1)/(2)N_(2)(g)+(3)/(2)H_(2)(g)

What is the mole percentage of O_(2) in a mixture of 7g of N_(2) and 8g of O_(2) ?

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 ?

108 g fairly concentrated solution of AgNO_(3) is electrolysed by using 0.1 F charge the mass of resulting solution is (a)94g (b)11.6g (c)96.4g (d)None of these

Let a function f be even and integrable everywhere and periodic with period 2. Let g(x)=int_0^x f(t) dt and g(t)=k The value of g(x+2)-g(x) is equal to (A) g(1) (B) 0 (C) g(2) (D) g(3)

One "mole" of NH_(4)HS(s) was allowed to decompose in a 1-L container at 200^(@)C . It decomposes reversibly to NH_(3)(g) and H_(2)S(g). NH_(3)(g) further undergoes decomposition to form N_(2)(g) and H_(2)(g) . Finally, when equilibrium was set up, the ratio between the number of moles of NH_(3)(g) and H_(2)(g) was found to be 3 . NH_(4)HS(s) hArr NH_(3)(g)+H_(2)S(g), K_(c)=8.91xx10^(-2) M^(2) 2NH_(3)(g) hArr N_(2)(g)+3H_(2)(g), K_(c)=3xx10^(-4) M^(2) Answer the following: What is the "mole" fraction of hydrogen gas in the equilibrium mixture in the gas phase?

One "mole" of N_(2) is mixed with three moles of H_(2) in a 4L vessel. If 0.25% N_(2) is coverted into NH_(3) by the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) , calculate K_(c) . Also report K_(c) for 1/2 N_(2)(g)+3/2 H_(2)(g) hArr NH_(3)(g)

One "mole" of NH_(4)HS(s) was allowed to decompose in a 1-L container at 200^(@)C . It decomposes reversibly to NH_(3)(g) and H_(2)S(g). NH_(3)(g) further undergoes decomposition to form N_(2)(g) and H_(2)(g) . Finally, when equilibrium was set up, the ratio between the number of moles of NH_(3)(g) and H_(2)(g) was found to be 3 . NH_(4)HS(s) hArr NH_(3)(g)+H_(2)S(g), K_(c)=8.91xx10^(-2) M^(2) 2NH_(3)(g) hArr N_(2)(g)+3H_(2)(g), K_(c)=3xx10^(-4) M^(2) Answer the following: To attain equilibrium, how much % by weight of folid NH_(4)HS got dissociated?

The total number of electrons in 2.0 g of D_(2)O to that in 1.8 g of H_(2)O

The equilibrium constant K_(c) for the reaction P_(4)(g)hArr 2P_(2)(g) is 1.4 at 400^(@)C. Suppose that 3 moles of P_(4)(g) and 2 moles of P_(2)(g) are mixed in 2 litre container at 400^(@)C. What is the value of reaction quotient (Q_(c)) ?