How many grams of co(g) are there in 74.5 ml of the gas at 0.933 atm and 30o c?

As per the given statement:

Using ideal gas law equation:

where

P represents the Pressure of a gas

V represents the Volume it occupies

R represents the Universal constant , usually given as:

R = 0.082 atm L/ mol k

First convert Celsius into Kelvin.

T = 273 + 30 = 303 K

Use conversion:

1 L = 1000 mL

V = 74.5 mL = L

Now substitute the given values we have;

Simplify:

n = 0.00279757305

or

n ≈0.0028 moles.

Since carbon monoxide, CO has molar mass of 28.01 g/mol

then;

g

Therefore, 0.078 g of CO(g) are there  in 74.5 mL of the gas at 0.933 atm and 30 degree C

a small container that holds a source of energy a solar cell that captures light energy and converts it into electricity a voltaic cell that uses the oxidation of a fuel to produce electricity

explanation: