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3 years ago

1 point

Chemistry

1 answer:

masya89 [10]3 years ago

8 0

Answer:

$V_2=1.34L$

Explanation:

Hello there!

In this case, since this problem is describing how pressure changes as a function of volume and vice versa, it is possible recall the Boyle's law as shown below:

$P_1V_1=P_2V_2$

Whereas we are asked to compute the volume when the change is pressure is performed (V₂); thus, we proceed as follows:

$V_2=\frac{P_1V_1}{P_2}\\\\V_2=\frac{1.55L*105.2kPa}{122.0kPa}\\\\V_2=1.34L$

Best regards!

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A student dissolves 15.0 g of ammonium chloride(NH4Cl) in 250. 0 g of water in a well-insulated open cup. She then observes the

iren2701 [21]

Answer:

1) Endothermic.

2) $Q_{rxn}=4435.04J$

3) $\Delta _rH=15.8kJ/mol$

Explanation:

Hello there!

1) In this case, for these calorimetry problems, we can realize that since the temperature decreases the reaction is endothermic because it is absorbing heat from the solution, that is why the temperature goes from 22.00 °C to 16.0°C.

2) Now, for the total heat released by the reaction, we first need to assume that all of it is released by the solution since it is possible to assume that the calorimeter is perfectly isolated. In such a way, it is also valid to assume that the specific heat of the solution is 4.184 J/(g°C) as it is mostly water, therefore, the heat released by the reaction is:

$Q_{rxn}=-(15.0g+250.0g)*4.184\frac{J}{g\°C}(16.0-20.0)\°C\\\\ Q_{rxn}=4435.04J$

3) Finally, since the enthalpy of reaction is calculated by dividing the heat released by the reaction over the moles of the solute, in this case NH4Cl, we proceed as follows:

$\Delta _rH=\frac{ Q_{rxn}}{n}\\\\\Delta _rH= \frac{ 4435.04J}{15.0g*\frac{1mol}{53.49g} } *\frac{1kJ}{1000J} \\\\\Delta _rH=15.8kJ/mol$

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viva [34]

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