According to the following reaction, how much energy is evolved during the reaction of 32.5 g b2h6 and 72.5 g cl2? the molar mass of b2h6 is 27.67 g/mol. b2h6(g) + 6 cl2(g) → 2 bcl3(g) + 6 hcl(g) δh°rxn = -1396 kj according to the following reaction, how much energy is evolved during the reaction of 32.5 g b2h6 and 72.5 g cl2? the molar mass of b2h6 is 27.67 g/mol. b2h6(g) + 6 cl2(g) → 2 bcl3(g) + 6 hcl(g) δh°rxn = -1396 kj a) 1640 kj b) 1430 kj c) 429 kj d) 3070 kj e) 238 kj.

The amount of heat evolved during the reaction is 238 kJ

Explanation:

To calculate the number of moles, we use the equation:

    .....(1)

Given mass of = 32.5 g

Molar mass of = 27.67 g/mol

Putting values in equation 1, we get:

Given mass of chlorine gas = 72.5 g

Molar mass of chlorine gas = 71 g/mol

Putting values in equation 1, we get:

For the given chemical equation:

By Stoichiometry of the reaction:

6 moles of chlorine gas reacts with 1 mole of

So, 1.021 moles of chlorine gas will react with = of

As, given amount of is more than the required amount. So, it is considered as an excess reagent.

Thus, chlorine gas is considered as a limiting reagent because it limits the formation of product.

Moles of reacted = 0.170 moles

Amount of heat released for 1 mole of = 1396 kJ

So, amount of heat released for 0.170 moles of

Hence, the amount of heat evolved during the reaction is 238 kJ

answer: the rate of diffusion increases with increase in temperature.

increase in temperature, increases the molecular/particles speed (kinetic energy. diffusion means movement of particles through the material.

generally, the heavier the particle the more it interacts with the environment and more the temperature matters. so higher temperature results in higher diffusion.