How many atoms are in a 2.70 cm × 2.70 cm × 2.70 cm cube of aluminum?

First, we calculate for the total volume of aluminum. The volume of a cube is:

V = s * s * s = s^3

V = (2.70 cm)^3

V = 19.683 cm^3

Assuming atmospheric temperature, the density of aluminum is about 2.70 g / cm^3. Therefore the equivalent mass of aluminum is:

m = 19.683 cm^3 * 2.70 g / cm^3

m = 53.1441 g

The molar mass of aluminum is 27 g / mol. Therefore the number of moles is:

n = 53.1441 g / (27 g / mol)

n = 1.9683 mol

Given the number of moles, we can calculate for the number of atoms using Avogadro’s number.

atoms = 1.9683 mol * (6.022 * 10^23 atoms / mol)

atoms = 11.85 * 10^23 atoms               (ANSWER)

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explanation:

force is based upon mass and acceleration.the statement is not always true.

it can be explained from newton's second law of motion.

as per newton's second law of motion the rate of change of momentum is directly proportional to the applied force and takes place along the direction of force.

mathematically it can be written as -

                                              ⇒      

here   k is the proportionality constant whose value is 1.

                                                            [a is the acceleration=dv/dt]

hence we see that force not only depends on mass and acceleration but also on velocity and rate of change of mass. force f will depend on mass and acceleration only when mass is constant.

hence the statement that force is based upon mass and acceleration is false.