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3 years ago

What is the energy change associated with 1.5 mole of D being formed?

Chemistry

1 answer:

AleksandrR [38]3 years ago

3 0

Answer:

–36 KJ.

Explanation:

The equation for the reaction is given below:

2B + C —› D + E. ΔH = – 24 KJ

From the equation above,

1 mole of D required – 24 KJ of energy.

Now, we shall determine the energy change associated with 1.5 moles of D.

This can be obtained as illustrated below:

From the equation above,

1 mole of D required – 24 KJ of energy

Therefore,

1.5 moles of D will require = 1.5 × – 24 = –36 KJ.

Therefore, –36 KJ of energy is associated with 1.5 moles of D.

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86.66 % by weight of ascorbic acid in the tablet, when 0. 1220 g vitamin c tablet was dissolved in acid. This required 11. 50 ml of 0. 01740 m $KIO_3$ to reach the endpoint.

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A balanced chemical reaction is an equation that has equal numbers of each type of atom on both sides of the arrow.

$3C_6H_80_6 +3I_2 +KIO_3 +5KI +6H^+$ → $3C_6H_60_6 +6I^- +3I_2+6K^+ +3H_2O$

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2 years ago

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3 years ago

What is the energy change associated with 1.5 mole of D being formed? ￼

What is the energy change associated with 1.5 mole of D being formed?