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Rudiy27
3 years ago
14

Which of the following describes an exothermic reaction?

Chemistry
2 answers:
Pavel [41]3 years ago
6 0

Answer:

The answer to your question is:  letter A

Explanation:

a) A + B ⇒ AB + heat     It is an exothermic reaction because heat is released.

b) A + BΔ ⇒ AB  It heat added to the reactants , then it is an endothermic reaction.

c) heat + BC ⇒ B + C  It's an endothermic reaction because heat is added to the reactants.

d) B + heat + CD ⇒ BD + C  It's and endothermic reaction because heat is added to the reactants.

viktelen [127]3 years ago
6 0

Answer:

The correct answer is a"

Explanation:

Hello! Let's solve this!

Exothermic reactions are those that release heat and endothermic reactions are those that consume heat.

a) A + B ⇒ AB + heat

It indicates that heat is released by what is an exothermic reaction.

b) A + BΔ ⇒ AB Heat is added to the reaction so it is endothermic

c) heat + BC ⇒ B + C

It is an endothermic reaction because heat is consumed in the reaction.

d) B + heat + CD ⇒ BD + C

It is an endothermic reaction since it consumes heat

The correct answer is a"

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How much heat is liberated at constant pressure when 1.41 g of potassium metal reacts with 6.52 mL of liquid iodine monochloride
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Answer:

The correct answer is -  13.33 kJ of heat

Explanation:

To know which one is the limiting reagent, determine the number of moles of each reagent in order .

n(K) = mass/atomic weight = 1.41/39 = 0.036 moles

Density of ICl = Mass/Volume

3.24 = Mass/6.52

Mass of ICl = 21.12 g

n(ICl) = mass/molar mass = 21.12/162.35 = 0.130 moles

2 moles of K reacts with 1 mole of ICl

0.036 moles of K will react with = 0.036/2 = 0.018 moles of ICl

since the amount of moles of ICl is more than 0.018, it is in excess and hence K is the limiting reagent. Now, use the balance equation to determine the amount of heat liberated:

2 moles of K gives out -740.71 kJ of heat

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0.036 moles of K will give out = 0.036 × 370.36 = 13.33 kJ of heat

Thus, the correct answer is -  13.33 kJ of heat

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