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astra-53 [7]
3 years ago
8

At 25°C and constant pressure, carbon monoxide gas combines with oxygen gas to give carbon dioxide gas with the evolution of 10.

1 kJ per gram of carbon monoxide consumed. What is the value of ΔH for the reaction as represented by the equation below.
Chemistry
1 answer:
stealth61 [152]3 years ago
4 0

Answer : The value of \Delta H for the reaction is, -565.6 kJ

Explanation :

First we have to calculate the molar mass of CO.

Molar mass CO = Atomic mass of C + Atomic mass of O  = 12 + 16 = 28 g/mole

Now we have to calculate the moles of CO.

\text{Moles of }CO=\frac{\text{Mass of }CO}{\text{Molar mass of }CO}=\frac{1g}{28g/mole}=\frac{1}{28}mole

Now we have to calculate the value of \Delta H for the reaction.

The balanced equation will be,

2CO(g)+O_2(g)\rightarrow 2CO_2(g)

From the balanced chemical reaction we conclude that,

As, \frac{1}{28}mole of CO release heat = 10.1 kJ

So, 2 mole of CO release heat = 2\times 28\times 10.1=565.6kJ

Therefore, the value of \Delta H for the reaction is, -565.6 kJ (The negative sign indicates the amount of energy is released)

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Given the mass of hydrogen = 16.0 oz

Converting 16.0 oz hydrogen to pounds (lb) using the conversion factor 1 lb = 16 oz:

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