The heat required to raise the temperature of 12g of water from 16 C to 21 C is: a) 60 J
b) 60 cal
c) 50 cal
d) 50 J

The correct option is;

b) 60 cal

Explanation:

The mass of the given water, m = 12 g

The initial temperature of he given water = 16°C

The final temperature of the given water = 21°C

The specific heat capacity of water, c = 4.184 J/(g·°C) = 1 cal/(g·°C)

The amount of heat, ΔQ, required = Mass × Specific heat capacity × Change in temperature

ΔQ = 12 × 4.184 × (21 - 16) = 251.04 J

Similarly, we have;

ΔQ = 12 g × 1 cal/(g·°C) × (21 - 16)°C = 60 cal

The amount of heat required = 60 cal.

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

it would be a gas formation