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IgorC [24]
3 years ago
7

Determine the number of moles of air present in 1.35 l at 750 torr and 17.0°c. ideal gas law formula: pv = nrt(r = 62.396 l•torr

/mol•k) which equation should you use? p equals startfraction n r t over v endfraction. n equals startfraction r t over p v endfraction. n equals startfraction p v over r t endfraction.
Chemistry
2 answers:
Tatiana [17]3 years ago
7 0

The number of moles of air present is 0.056 mole

<h3>What is the ideal gas equation?</h3>

The ideal gas is one in which molecules do not attract or repel each other.Many gases like oxygen,nitrogen, carbon di oxide can be treated as the ideal gases as particular temperature and pressure.The real gases at high temperature and lower pressure can be treated as ideal gases.

The given data in the question is

Volume = 1.35 L

Pressure (P) = 750 torr

Temperature (T) = 17 °C = 17 + 273 = 290 K

Gas constant (R) = 62.396 L•torr/mol•K

The number of moles (n) =?

How to determine the number of moles:

The number of moles present can be obtained by using the ideal gas equation as illustrated below:

PV=nRT

Divide both sides by RT

n=\dfrac{PV}{RT}

n=\dfrac{(750\times 1.350}{62.396\times 290)}

n=0.056\ moles

Hence, the number of moles of air present is 0.056 mole

To learn more about the ideal gas equation follow

brainly.com/question/4147359

aliina [53]3 years ago
7 0

Answer:

answer in picture

Explanation:

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For every mole of SO_{2} we would need twice of H_{2}S moles, so for every 3 moles of S_{8} we need 16 moles of H_{2}S


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2.61 X (3/16) = 0.49 moles


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Explanation :

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The given final reaction is,

Fe_2O_3(s)+3CO(g)\rightarrow 2Fe(s)+3CO_2(g)    \Delta H=?

The intermediate balanced chemical reaction will be,

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(2) CO(g)+\frac{1}{2}O_2(g)\rightarrow CO_2(g)    \Delta H^o_2=-282.7kJ

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The expression for final enthalpy is,

\Delta H=\Delta H^o_1+\Delta H^o_2

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