A 0.982-g sample of an unknown gas exerts a pressure of 700 mm Hg in a 450-cm3 container at 23oC. Calculate the molar mass of this gas. [1cm3 = 1mL; 1000mL = 1L]

57.4 g/mol

Explanation:

Step 1: Convert 450 cm³ to L

We will use the conversion factors 1 cm³ = 1 mL and 1000 mL = 1 L.

450 cm³ × 1 mL/1 cm³ × 1 L/1 mL = 0.450 L

Step 2: Convert 23 °C to Kelvin

We will use the following expression.

K = °C + 273.15 = 23 + 273.15 = 296 K

Step 3: Calculate the number of moles of the gas

We will use the ideal gas equation.

P × V = n × R × T

n = P × V / R × T

n = 700 mmHg × 0.450 L / (62.4 mmHg.L/mol.K) × 296 K = 0.0171 mol

Step 4: Calculate the molar mass of the gas

0.982 g of the gas correspond to 0.0171 moles.

M = 0.982 g/0.0171 mol = 57.4 g/mol

fire could start, buildings collapsing, and ash falling from the sky.

explanation:

this is because the buildings or plants could catch on fire and the buildings would most likely collapse. lastly ash would fall because all the burning would cause ash to fall from the sky.

hope this .

your answer would be a. 12.5 kg