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Alexeev081 [22]
2 years ago
10

When the mixture was moved from room temperature to a higher temperature, the mixture turned darker brown. Which of the followin

g conclusions about the mixture is true?
The forward reaction is exothermic.
The backward reaction has a negative net enthalpy.
The colorless gas has a higher enthalpy than the brown gas.
The equilibrium between the two forms of the gas is disturbed at high temperatures.
Chemistry
1 answer:
Wittaler [7]2 years ago
7 0

Answer:

The equilibrium between the two forms of the gas is disturbed at high temperatures.

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A resting adult requires about 240 ml of pure oxygen/mind and breathes about 12 times every minute. if inhaled air contains 20 p
Dmitry_Shevchenko [17]

12 times breathe give 240 ml of pure O_{2}. Each breathe gives 20 ml of O_{2}.

Let us consider, volume of air per breathe= x ml.

Pure O_{2} from inhaled air= \frac{20}{100}x ml and Pure O_{2} from exhaled air= \frac{16}{100}x ml.

Pure O_{2} from inhaled and exhaled air= 20 ml

So, \frac{20}{100}x + \frac{16}{100}x = 20

Therefore, x = 55.5 ml

So, volume of air per breath= 55.5 ml.


7 0
3 years ago
How much heat does a 100. g sample of copper absorb when its temperature increases by 30.0°C? The specific heat of copper is 0.3
erica [24]

Answer:

\boxed {\boxed {\sf B. \ 1170 \ Joules }}

Explanation:

We are asked to find how much heat a sample of copper absorbs when the temperature is increased.

Since we know the mass, temperature increase, and specific heat capacity, we can use the following formula to calculate heat.

q= mc \Delta T

The mass of the copper sample is 100 grams, the temperature is changed or increased by 30.0 degrees Celsius, and the specific heat of copper is 0.39 Joules per gram degrees Celsius.

  • m= 100 g
  • c= 0.39 J/g °C
  • ΔT= 30.0 °C

Substitute the values into the formula.

q= (100 \ g )(0.39 \ J/g \textdegree C ) (30.0 \textdegree C )

Multiply the first two values. Note that the units of grams cancel.

q= 39 \ J/ \textdegree C (30.0 \textdegree C )

Multiply again, this time the units of degrees Celsius cancel.

q= 1170 \ J

The copper sample absorbs <u>1170 Joules</u> of heat and <u>Choice B </u>is correct.

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Explanation:

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