The molar mass of this gas is 92.3 g/mol

Calculation

By use ideal gas equation PV =nRT where
n=mole p=pressure V= volume R = gas constant T= temperature

n = mass /molar mass(MM)
substitute in the equation

PV =(mass/MM)RT
mass = density x volume(V)

Therefore PV =(density xV/ MM) xRT

divide both side by by V

P= (density/Mm) xRT

making MM the subject of the formula

MM = densityPRT

At STP = P= 1 atm, R= 0.0821 L.atm/Mol.k T = 273 K

MM is therefore = 4.12 g/l x 1 atm x 0.081 L.atm/mol.k x 273 K = 92.3 g/mol

7 0

2 years ago

Read 2 more answers

A) How much CO is required for the production of Fe from 1000 tonnes of magnetite (Fe2O4). Assume that the iron ore is 100% pure

Kryger [21]

Its b im pretty sure

5 0

2 years ago

If a sample of HF gas at 694.9 mmHg has a volume of 3.463 Land the volume is changed to 5.887 L, then what will be the new press

VARVARA [1.3K]

Answer:

$\large \boxed{\text{381.7 mmHg}}$

Explanation:

Data:

p₁ = 694.9 mmHg; V₁ = 3.463 L

p₂ = ?; V₂ = 5.887 L

Calculation:

$\begin{array}{rcl}p_{1}V_{1} & = & p_{2}V_{2}\\\text{648.9 mmHg} \times \text{3.463 L} & = & p_{2} \times\text{5.887 L}\\\text{2247.1 mmHg} & = & 5.887p_{2}\\p_{2} & = & \dfrac{\text{2247.1 mmHg}}{5.887}\\\\& = &\textbf{381.7 mmHg}\\\end{array}\\\text{The new pressure of the gas is $\large \boxed{\textbf{381.7 mmHg}}$}$

4 0

3 years ago