Question

Consider these reactions:
Reaction 1: H2(g) + Cla (g)
2HC1(g) AH = -184.6 kJ

Reaction 2: 20F2(g)
02(g) + 2 F2(g)
AH = -49.4 kJ

Reaction 3: N2(g) + 202(g)
2N02(g)
AH = +66.4 kJ

Use Reaction 1.

Determine the mass, in grams, of chlorine gas consumed (with excess H-) when
1,342.0 kJ of energy iS released from the system.
Answer: g

Answer 1

511.2 grams of chlorine gas consumed (with excess H-) when

1,342.0 kJ of energy is released from the system.

What is an exothermic reaction?

In thermochemistry, an exothermic reaction is a "reaction for which the overall standard enthalpy change ΔH⚬ is negative."

Given that 1 mole of chlorine releases -184.6 energy.

Then, we have to find the number of moles of chlorine when 1,342.0 kJ of energy is released from the system.

So, calculating number of moles of chlorine.

Moles = $\frac{-1,342.0 \;kJ}{-184.6\;kJ}$

Moles = 7.2 mole

Now, calculating number mass of chlorine.

$\rm Moles=\rm\frac{Mass}{Molar \;mass}$

Mass =  7.2 mole x 71 g/mole

Mass = 511.2 gram

Learn more about exothermic reaction here:

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