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fomenos
3 years ago
15

A 5.00 l sample of a gas exerts a pressure of 1040 torr at 50.0°c. In what volume would the same sample exert a pressure of 1.00

atm at 50.0°c?
Chemistry
1 answer:
Karolina [17]3 years ago
8 0

Answer: 7L

Explanation:

To calculate the new volume, we use the equation given by Boyle's law. This law states that pressure is directly proportional to the volume of the gas at constant temperature.  

The equation given by this law is:

P_1V_1=P_2V_2

where,

P_1\text{ and }V_1 are initial pressure and volume.

P_2\text{ and }V_2 are final pressure and volume.

We are given:

P_1=1040torr=1.4atm(1torr=0.0013atm)\\V_1=5.00L\\P_2=1atm\\V_2=?

Putting values in above equation, we get:

1.4\times 5.0L=1atm\times V_2\\\\V_2=7L

The volume would be 7L at pressure of 1.00 atm at 50.0°C.

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How much heat is required to convert 20.0 g of ice at 50.0⁰C to liquid water at 0.0⁰C? The specific heat of ice is 2.06 J/(g∙⁰C)
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8740 joules are required to convert 20 grams of ice to liquid water.

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The amount of heat required (Q), measured in joules, to convert ice at -50.0 ºC to liquid water at 0.0 ºC is the sum of sensible heat associated with ice and latent heat of fussion. That is:

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m - Mass, measured in grams.

c - Specific heat of ice, measured in joules per gram-degree Celsius.

T_{o}, T_{f} - Temperature, measured in degrees Celsius.

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If we know that m = 20\,g, c = 2.06\,\frac{J}{g\cdot ^{\circ}C}, T_{f} = 0\,^{\circ}C, T_{o} = -50\,^{\circ}C and L_{f} = 334\,\frac{J}{g }, then the amount of heat is:

Q = (20\,g)\cdot \left\{\left(2.06\,\frac{J}{g\cdot ^{\circ}C} \right)\cdot [0\,^{\circ}C-(-50\,^{\circ}C)]+334\,\frac{J}{g} \right\}

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8740 joules are required to convert 20 grams of ice to liquid water.

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