Which products are formed during the decomposition of magnesium nitride (mg3n2)? a. mg + 3n2 b. 3mg + 2n2 c. mg + 3n d. 3mg + n2 e. 2mg + 3n

Decomposition reactions involve the breaking down of compounds to form smaller molecules or elements.

Thus, magnesium nitride will decompose to form elemental magnesium and nitrogen gas

Mg₃N₂  → Mg + N₂

The reaction now needs to be balanced, such that the number of Mg and N atoms in the reactants is equal to that of the products.

Balanced reaction:

Mg₃N₂ → 3Mg + N₂

Ans (D)

The product   that are  formed   during  the decomposition  of magnesium nitride    is   3Mg + N2  ( answer D)

    Explanation

  magnesium  nitride   decompose  to form  magnesium  and nitrogen  according to   equation below.

 Mg3N2  → 3Mg  +N2

According to reaction above  1 mole of Mg3N2  decomposes  to  form     3  moles of Mg  and  1   moles  of N2

when 25.0 ml of 0.700 mol/l naoh was mixed in a calorimeter with 25.0 ml of 0.700 mol/l hcl, both initially at 20.0 °c, the temperature increased to 22.1 °c. the heat capacity of the calorimeter is 279 j/°c.

the equation for the reaction is:

naoh + hcl → nacl + h₂o

moles of hcl = 0.0250 l hcl ×

0.700

mol hcl

1 l hcl = 0.0175 mol hcl

volume of solution = (25.0 + 25.0) ml = 50.0 ml

mass of solution = 50.0 ml soln ×

1.00

ml soln

= 50.0 g soln

δt=t2-t1

= (22.1 – 20.0) °c = 2.1 °c

the heats involved are

heat from neutralization + heat to warm solution + heat to warm calorimeter = 0

q1+q2+q3=0

nδh+mcδt+cδt=0

0.0175 mol ×

δh

+ 50.0 g × 4.184 j·g⁻¹°c⁻¹ × 2.1 °c + 279 j°c⁻¹ × 2.1 °c = 0

0.0175 mol ×

δh

+ 439.32 j + 585.9 j = 0

0.0175 mol ×

δh

= -1025.22 j

δh=1025.22j0.0175 mol= -58 600 j/mol = -58.6 kj/mol