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In-s [12.5K]
3 years ago
13

Radio waves travel at the speed of light, which is 3X10^8 m/s. How many minutes does it take for a radio message to reach earth

from Saturn if Saturn is 7.9X10^8 km from earth?
Chemistry
1 answer:
Mandarinka [93]3 years ago
4 0

Answer:

43.89 min

Explanation:

Given that:-

The speed of light = 3.00\times 10^8\ m/s

The distance = 7.9\times 10^8\ km

The conversion of distance in km to distance into m is shown below as:-

1 km = 1000 m

So,  

Distance = 7.9\times 10^8\times 1000\ m=7.9\times 10^{11}\ m

The relation between speed distance and time is shown below as:-

Speed=\frac{Distance}{Time}

Thus,  

3.00\times 10^8=\frac{7.9\times 10^{11}}{Time}

300000000\times time=10^{11}\times \:7.9\ s

Time = 2633.33 seconds

Also, 1 s = 1/60 min

So,  

Time=\frac{2633.33}{60}\ min=43.89\ min

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Answer:

B

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What is the final volume of a 400 ML sample that is subjected To a temperature change from 22 Celsius to 30 Celsius in a pressur
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Answer:

The answer to your question is  V2 = 867.3 mL

Explanation:

Data

Volume 1 = V1 = 400 ml

Temperature 1 = T1 = 22°C

Pressure 1 = P1 = 760 mmHg

Volume 2 = V2 = ?

Temperature 2 = T2 = 30°C

Pressure 2 = P2 = 360 mmHg

Process

1.- Convert Celsius to Kelvin

T1 = 22 + 273 = 295°K

T2 = 30 + 273 = 303°K

2.- Use the Combined gas law

              P1V1/T1 = P2V2/T2

- Solve for V2

            V2 = P1V1T2 / T1P2

- Substitution

            V2 = (760 x 400 x 303) / (295 x 360)

- Simplification

            V2 = 92112000 / 106200

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3 years ago
Tetrahydrofuran (THF) is a common organic solvent with a boiling point of 339 K. Calculate the total energy (q) required to conv
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Explanation:

For the given reaction, the temperature of liquid will rise from 298 K to 339 K. Hence, heat energy required will be calculated as follows.

             Q_{1} = mC_{1} \Delta T_{1}

Putting the given values into the above equation as follows.

           Q_{1} = mC_{1} \Delta T_{1}

                      = 27.3 g \times 1.70 J/g K \times 41

                      = 1902.81 J

Now, conversion of liquid to vapor at the boiling point (339 K) is calculated as follows.

           Q_{2} = energy required = mL_{v}

    L_{v} = latent heat of vaporization

Therefor, calculate the value of energy required as follows.

             Q_{2} = mL_{v}

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Therefore, rise in temperature of vapor from 339 K to 373 K is calculated as follows.

            Q_{3} = mC_{2} \Delta T_{2}

Value of C_{2} = 1.06 J/g,    \Delta T_{2} = (373 -339) K = 34 K

Hence, putting the given values into the above formula as follows.

             Q_{3} = mC_{2} \Delta T_{2}

                       = 27.3 g \times 1.06 J/g \times 34 K

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Therefore, net heat required will be calculated as follows.

            Q = Q_{1} + Q_{2} + Q_{3}

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                = 15007.902 J

Thus, we can conclude that total energy (q) required to convert 27.3 g of THF at 298 K to a vapor at 373 K is 15007.902 J.

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