Gravitational potential energy (U) = mgh = 2 kg * 9.8 m/s^2 * 10 m = 196 J.

U = mgh = 2 * 9.8 * 10 = 196 J.

Using U = mgh, U = 2 kg * 9.8 m/s^2 * 5 m = 98 J.

Potential Energy PE = m * g * h = 2 kg * 9.8 m/s² * 5 m = 98 J

Gravitational potential energy U = mgh = 5 * 9.8 * 10 = 490 J.

The gravitational potential energy U at height h is given by U = mgh.

The gravitational potential energy is given by the formula U = mgh, where g is the acceleration due to gravity.

Gravitational potential energy U = mgh = 10 * 9.8 * 5 = 490 J.

Gravitational potential energy U = mgh = 10 kg * 9.8 m/s² * 5 m = 490 J, approximately 500 J.

U = mgh = 10 * 9.8 * 5 = 490 J

Gravitational potential energy (U) = mgh = 2 kg * 9.8 m/s^2 * 10 m = 196 J.

The gravitational potential energy of a satellite at height h is given by U = -GMm/(R+h), where R is the radius of the Earth.

The gravitational potential energy is given by the formula U = mgh.

The gravitational potential energy is given by U = -G * (m1 * m2) / r.

The gravitational potential energy is given by U = -G * (m1 * m2) / r.

The half-life is defined as the time taken for half of the radioactive sample to decay.

The half-life is defined as the time required for half of the radioactive substance to decay, which is given as 10 years.

The half-life of a radioactive substance is defined as the time taken for half of the substance to decay.

A tetrahedral shape corresponds to sp3 hybridization.

The nitrogen in a primary amine is sp3 hybridized.

Nitrogen in amines is sp3 hybridized due to the presence of three substituents and a lone pair.

In acetylene, each carbon atom is sp hybridized, forming a triple bond between them.

In CO2, the carbon atom forms two double bonds with oxygen atoms, indicating sp hybridization.

In ethylene, each carbon atom is sp2 hybridized, forming a double bond with the other carbon.

The carbon atoms in ethyne (C2H2) are sp hybridized due to the triple bond between them.

In alkynes, the carbon atoms involved in the triple bond are sp hybridized.

The carbon atoms in benzene are sp2 hybridized, forming a planar structure with 120-degree bond angles.

The carbon atoms in ethylene (C2H4) are sp2 hybridized due to the presence of a double bond.

In ethyne, the carbon atoms are sp hybridized due to the presence of a triple bond.

The carbon atoms in the double bond of alkenes are sp2 hybridized.