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3 years ago

Give the ΔH value for the formation of binary compounds as shown in the reaction H2(s)+Br2(g)→2HBr(s)+36.3kJ.

Chemistry

1 answer:

Amanda [17]3 years ago

8 0

Answer:

ΔH = - 36.3 kJ

Explanation:

The given chemical reaction is as follows -

H₂ (s) + Br₂ (g) ------> 2HBr (s) + 36.3 kJ

In the above equation , the amount of energy i.e. 36.3 kJ is released , i.e. it is in the product side , hence , the reaction is an example of an exothermic reaction .

Hence ,

The value of the change in enthalphy , i.e. , the enthalpy of product minus the enthalpy of the product .

Therefore ,

The value of the change in enthalphy = - ve .

Hence ,

ΔH = - 36.3 kJ

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What is the mass present in a 10.0L container of oxygen at a pressure of 105kPa and 20 degrees Celsius

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<h3>Explanation</h3>

Assume that oxygen acts like an ideal gas. In other words, assume that the oxygen here satisfies the ideal gas law:

$P \cdot V = n \cdot R\cdot T$ ,

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$P$ the pressure on the gas, $\bf P = 10^{5}\;\textbf{kPa}=10^{8}\;\textbf{Pa}$ ;
$V$ the volume of the gas, $V = 10.0 \;\text{L} = 10.0\times 10^{-3}\;\text{m}^{3}=10^{-2}\;\text{m}^{3}$ ;
$n$ the number of moles of the gas, which needs to be found;
$T$ the absolute temperature of the gas, $T=20\;\textdegree{}\text{C} = (20 + 273.15)\;\text{K} = 293.15\;\text{K}$ .
$R$ the ideal gas constant, $R = 8.314$ if P, V, and T are in their corresponding SI units: Pa, m³, and K.

Apply the ideal gas law to find $n$ :

$n = \dfrac{P\cdot V}{R\cdot T} = \dfrac{{\bf 10^{8}\;\textbf{Pa}}\times 10^{-2}\;\text{m}^{3}}{8.314 \;\text{Pa}\cdot\text{m}^{3}\cdot\text{K}^{-1}\cdot\text{mol}^{-1}\times 293.15\;\text{K}} = 410.3\;\text{mol}$ .

In other words, there are 410.3 moles of O₂ molecules in that container.

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$410.3 \times 32.00 = 1.31\times10^{4}\;\text{g}$ .

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