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sesenic [268]
3 years ago
11

A gas sample has an initial volume of 63.2 mL, an initial temperature of 42.0 ?C, and an initial pressure of 751 mmHg. The volum

e is decreased to 47.6 mL and the temperature is increased to 77.0 ?C.
Chemistry
1 answer:
exis [7]3 years ago
4 0

Answer:

Lets Write Down the Given Initial Conditions.

P_1 = 751mmHg           P_2 = --

V_1 = 63.2ml                V_2 = 47.6ml

T_1 = 42C                     T_2 = 77

In Order to Solve for the Unknown: P_2

we must use the Ideal Gas Law to Solve for the Second Unknown pressure:

\frac{P_1V_1}{T_1} =\frac{P_2V_2}{T_2}

Then Rearrange this equation in a form where P2 can be solved from:

P_2 = \frac{P_1V_1T_2}{T_1V_2}

Then Insert the Values from above to solve:

P_2 = \frac{(751 mmHg)(63.2ml)(77C)}{(47.6ml)(42C)}

The Answer is : 1830 mmHg considering sig figs

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