2.9g of gas at 95°C occupied the same volume as 0.184g of hydrogen at 17°C at the same pressure. What is the molar mass of the gas ?

Subject:
Chemistry
Author:
aldo
Created:
1 year ago

Answers 2

Answer:

40 g mol–1

Explanation:

2.9 g of a gas at 95 °C occupied the same volume as 0.184g of dihydrogen at 17 °C, at the same pressure.Hence, the molar mass of the gas is 40 g mol–1.

Author:

jakepham
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Answer:

The molar mass of the gas is 40gmol⁻¹.

Explanation:

Given,

mass of H₂ = 0.184g

mass of gas = 2.9g

Temperature of H₂, T₁ = 17°C = 17+273 =290K

Temperature of gas, T₂ = 95°C = 95+273 =368K

moles of H₂ , n₁ = mass of H₂ / molar mass of H₂

⇒ = 0.184g / 2gmol⁻¹ = 0.092mol.

the ideal gas equation is,

PV = nRT

Since P and V is constant,

⇒ PV/R is constant

⇒ nT is constant

then we can write,

n₂ T₂= n₁ T₁

moles of gas, n₂ = n₁ × (T₁ / T₂)

⇒ = 0.092 × (290/368) = 0.0725mol.

molar mass of gas = mass of gas /moles of gas

⇒ = 2.9 / 0.0725 = 40gmol⁻¹

Hence, the required answer is 40gmol⁻¹.

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rainaondg
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2.9g of gas at 95°C occupied the same volume as 0.184g of hydrogen at 17°C at the same pressure. What is the molar mass of the gas ?

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2.9g of gas at 95°C occupied the same volume as 0.184g of hydrogen at 17°C at the same pressure. What is the molar mass of the gas ?​

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2.9g of gas at 95°C occupied the same volume as 0.184g of hydrogen at 17°C at the same pressure. What is the molar mass of the gas ?