The correct answer to the top one is d
- hands start getting sweaty
- nail biting or perhaps shaking legs
- the feeling of being overwhelmed
- (for some people) the stomach starts to hurt
Answer:
323.15 °C
Explanation:
Considering the ideal gas equation as:

where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Thus, at constant volume and number of moles, Pressure of the gas is directly proportional to the temperature of the gas.
P ∝ T
Also,
Using Charle's law
Given ,
P₂ = 2P₁
T₁ = 25 °C
T₂ = ?
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T₁ = (25 + 273.15) K = 298.15 K
Using above equation as:
New temperature = 596.3 K
Also,
T(K) - 273.15 = T( °C)
<u>So, Temperature = 596.3 - 273.15 °C = 323.15 °C</u>
Answer:
H2-1
H2+-1/2
H22- zero
Explanation:
Bond order= Bonding electrons-antibonding electrons/2
In H2, there are two bonding electrons and no antibonding electrons. In H2+ there is only one bonding electron and no antibonding electron while in H22- there are two bonding and two antibonding electrons respectively.
Atomic weight of an element can be calculated as follows:
average atomic weight =
(atomic weight of first isotope)(its percentage of abundance) +
(atomic weight of second isotope)(its percentage of abundance)
average atomic weight = 98.225 amu
atomic weight of first isotope = 97.780 amu
its percentage of abundance = 1 - 0.417 = 0.583
atomic weight of second isotope = ??
its percentage of abundance = 0.417
So, just substitute in the above equation to get the atomic weight of the second isotope as follows:
98.225 = (97.78)(0.583) + (mass2)(0.417)
atomic weight of second isotope = 98.847 amu