Answer:
For example, the relative rate of a reaction at 20 seconds will be 1/20 or 0.05 s -1, while the average rate of reaction over the first 20 seconds will be the change in mass over that period, divided by the change in time.
Explanation:
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Answer: The volume occupied by 2.50 moles of
gas at STP is 56.0L
Explanation:
According to ideal gas equation:

P = pressure of gas = 1 atm (at STP)
V = Volume of gas = ?
n = number of moles = 2.50
R = gas constant =
T =temperature =
(at STP)


Thus the volume occupied by 2.50 moles of
gas at STP is 56.0L
First, we have to calculate the number of moles of H2SO4 in the solution:
V=60 mL = 0.06 L
c=5.85 mol/L
n=V×c=0.06×5.85=0.351 mol
Then we need to find the molar mass of H2SO4:
2×Ar(H) + Ar(S) + 4×Ar(O) =
=2 + 32 + 64 = 98 g/mol
Finally, we need to find the mass of H2SO4:
m=0.351 × 98 = 34.398 g
<span>I think There should be a valanced state in every atom. (Valanced state means, 8 electrons in the outer most orbit) In case take a atom has 8 electrons in the outer orbit, so when bonding the two atom to form a molecule, there is a Ionic Bond (because of both atoms has its own valanced electron(8 electrons in outer most orbit).</span>
Answer : The thermal energy produced during the complete combustion of one mole of cymene is -7193 kJ/mole
Explanation :
First we have to calculate the heat released by the combustion.

where,
q = heat released = ?
= specific heat of calorimeter = 
= change in temperature = 
Now put all the given values in the above formula, we get:


Thus, the heat released by the combustion = 70.43 kJ
Now we have to calculate the molar enthalpy combustion.

where,
= molar enthalpy combustion = ?
q = heat released = 70.43 kJ
n = number of moles cymene = 

Therefore, the thermal energy produced during the complete combustion of one mole of cymene is -7193 kJ/mole