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3 years ago

28. If the total pressure of a mixture of four gases (neon, carbon dioxide, oxygen and hydrogen) is 1245 mm

Chemistry

1 answer:

Bingel [31]3 years ago

8 0

Answer:

D) 373 mm Hg.

Explanation:

We can solve this problem by keeping in mind Dalton's law of partial pressures, which states that the total pressure of a mixture of gases is equal to the sum of each gas' partial pressures. In other words, for this case:

Total Pressure = Ne Pressure + CO₂ Pressure + O₂ Pressure + H₂ Pressure

1245 mm Hg = Ne Pressure + 145 mm Hg + 228 mm Hg + 499 mm Hg

Ne Pressure = 373 mm Hg

The answer is option D) 373 mm Hg.

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Answer:

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2 years ago

Given 6193 mL of a gas at 62.3 °C. What is its volume at 38.1 °C?

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Answer:

5746.0 mL.

Explanation:

We can use the general law of ideal gas: PV = nRT.

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R is the general gas constant,

T is the temperature of the gas in K.

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V₁T₂ = V₂T₁

V₁ = 6193.0 mL, T₁ = 62.3°C + 273 = 335.3 K.

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3 years ago

A tank holds 6.90 m3 of water. What is the volume in ft3? (3.28 ft = 1 m, Remember significant figures, but this answer does not

AleksAgata [21]

Volume of tank = $6.9 m^{3}$ (given)

Since, $1 m = 3.28 ft$

So,

$1 m^{3} = 35.287 ft^{3}$

For $6.9 m^{3}$ :

$6.9\times 35.287 ft^{3} = 243.4803 ft^{3}$

The significant rule for multiplication, states that the number of significant figures in the answer obtained by multiplication is determined by the value with the lowest number of significant digits.

Since, the minimum number of decimal places in the above multiplication operation is 1 so, the final result must be upto 1 decimal place only.

$243.4803 ft^{3} \simeq 243.5 ft^{3}$