In a water molecule, the shared electrons spend more time around

The first two ionization energies of nickel.

Radda [10]

The first two ionization energy of nickel are expressed as:
Ni(g) = Ni^+(g) + e^- Ni^+(g) = Ni^2+(g) + e^-
IOnization energy os the energy that is neccessary in order to remove one mole of electrons from an atom.
Hope this helps.

7 0

4 years ago

What is a flame,metion two types of flames

12345 [234]

Answer:

A flame is defined as the gaseous part of the fire which is visible to us. A flame is created due to the high exothermic reaction.

Two types of flames based on the amount of oxygen available are:

Non-luminous or blue flame: In this type of flame the amount of oxygen is sufficiently large and it gives blue flame. For example: flame of Gas stove.
Luminous flame: In this type of flame, the oxygen availability id not sufficient for the complete combustion and left unburnt carbon particles that forms yellow light flame. For example: kerosene lamp.

7 0

3 years ago

How much energy (heat) is required to convert 248 g of water from 0 oC to 154 oC? Assume that the water begins as a liquid, that

Nuetrik [128]

Answer:

The total heat required is 691,026.36 J

Explanation:

Latent heat is the amount of heat that a body receives or gives to produce a phase change. It is calculated as: Q = m. L

Where Q: amount of heat, m: mass and L: latent heat

On the other hand, sensible heat is the amount of heat that a body can receive or give up due to a change in temperature. Its calculation is through the expression:

Q = c * m * ΔT

where Q is the heat exchanged by a body of mass m, constituted by a substance of specific heat c and where ΔT is the change in temperature (Tfinal - Tinitial).

In this case, the total heat required is calculated as:

Q for liquid water. This is, raise 248 g of liquid water from O to 100 Celsius. So you calculate the sensible heat of water from temperature 0 °C to 100° C

Q= c*m*ΔT

$Q=4.184\frac{J}{g*C} *248 g* (100 -0 )C$

Q=103,763.2 J

Q for phase change from liquid to steam. For this, you calculate the latent heat with the heat of vaporization being 40 and being 248 g = 13.78 moles (the molar mass of water being 18 g / mol, then $\frac{248 g}{18 \frac{g}{mol} } =13.78 moles$ )