A280 ml bubble contains 0.283 g of a gas at 0.951 atm and 25.0°c what is the molar mass of this gas?

28.3 g/mol

Explanation:

According to the ideal gas equation:'

P= Pressure of the gas = 0.951 atm

V= Volume of the gas = 280 mL = 0.28 L     (1L=1000 ml)

T= Temperature of the gas = 25°C=(25+273)K=298 K   (0°C = 273 K)

R= Value of gas constant = 0.0821 Latm/K mol

To calculate the moles, we use the equation:

Thus the molar mass of the gas is 28.3 g/mol.

c (diamond),

sio2 (quartz)

the density of gold = 19.3 g/cm3

the relation between density and mass and volume is

density = mass / volume

given :

mass of gold = 13 g

density = 13g / volume = 19.3

volume = 13 /19.3 = 0.67 cm^3

thus volume of gold nugget = 0.67 cm^3