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Nitrogen gas and oxygen can combine to produce nitric oxide such a reaction absorbs 88KJ of heat from the surroundings, how many grams of nitrogen gas do you predict were consumed in the reaction?N2 + O2 -> 2NO. AH=180kJ

Sagot :

N2 (g) + O2 (g) =======> 2 NO (g) AH = 180kJ

Don't forget to balance the reaction.

This is an endothermic reaction because it needs heat to produce and the sign + of AH

Some reactions absorb enthalpy and others free heat.

We can find the mass of N2 using this enthalpy:

N2 (g) + O2 (g) =======> 2 NO (g) AH = 180kJ

x (grams) AH = 88 kJ

First, we calculate the molecular mass of N2:

Molar mass N2 = 28.01 g / mole so,

1 mol N2 = 28.01 g N2

Now:

28.01 g of N2 ----------------------- absorb 180kJ (stoichiometry)

x (we need this)----------------------- 88 kJ (is real)

[tex]x=\text{ }\frac{88kJ\text{ . 28.01 g N2}}{180kJ\text{ }}=13.69\text{ g of N2}[/tex]

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