I2 + F2 = IF7

I_2 (iodine) + F_2 (fluorine) ⟶ F_7I_1 (iodine heptafluoride)

Balance the chemical equation algebraically: I_2 + F_2 ⟶ F_7I_1 Add stoichiometric coefficients, c_i, to the reactants and products: c_1 I_2 + c_2 F_2 ⟶ c_3 F_7I_1 Set the number of atoms in the reactants equal to the number of atoms in the products for I and F: I: | 2 c_1 = c_3 F: | 2 c_2 = 7 c_3 Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c_1 = 1 and solve the system of equations for the remaining coefficients: c_1 = 1 c_2 = 7 c_3 = 2 Substitute the coefficients into the chemical reaction to obtain the balanced equation: Answer: | | I_2 + 7 F_2 ⟶ 2 F_7I_1

+ ⟶

iodine + fluorine ⟶ iodine heptafluoride

K_c = [F7I1]^2/([I2] [F2]^7)

rate = -(Δ[I2])/(Δt) = -1/7 (Δ[F2])/(Δt) = 1/2 (Δ[F7I1])/(Δt) (assuming constant volume and no accumulation of intermediates or side products)

| iodine | fluorine | iodine heptafluoride formula | I_2 | F_2 | F_7I_1 Hill formula | I_2 | F_2 | F_7I name | iodine | fluorine | iodine heptafluoride IUPAC name | molecular iodine | molecular fluorine | heptafluoro-$l^{7}-iodane

| iodine | fluorine | iodine heptafluoride molar mass | 253.80894 g/mol | 37.996806326 g/mol | 259.89329 g/mol phase | solid (at STP) | gas (at STP) | melting point | 113 °C | -219.6 °C | boiling point | 184 °C | -188.12 °C | density | 4.94 g/cm^3 | 0.001696 g/cm^3 (at 0 °C) | solubility in water | | reacts | dynamic viscosity | 0.00227 Pa s (at 116 °C) | 2.344×10^-5 Pa s (at 25 °C) |