Given:
m = 52 kg. the mass of water
ΔT = 22 °C, the temperature increase
Note that
c = 4.184 J/(g-°C), the specific heat of water.
The quantity of heat required is
Q = mcΔT
= (52,000 g)*(4.184 J/(g-°C))*(22 °C)
= 4.7865 x 10⁴ J
Because 1 J = 2.39 x 10⁻⁴ cal. the heat required is
Q = (4.7865 x 10⁴ J)*(2.39 x 10⁻⁴ cal/J) = 1143.97 cal ≈ 1144 cal
Answer: 1144 cal
A reaction in which Oxygen (O₂) is produced from Mercury Oxide (HgO) would be a decomposition reaction.
2HgO → 2Hg + O₂
If 250g of O₂ is needed to be produced,
then the moles of oxygen needed to be produced = 250g ÷ 32 g/mol
= 7.8125 mol
Now, the mole ratio of Oxygen to Mercury Oxide is 1 : 2
∴ if the moles of oxygen = 7.8125 mol
then the moles of mercury oxide = 7.8125 mol × 2
= 15.625 mol
Thus the number moles of HgO needed to produce 250.0 g of O₂ is 15.625 mol
Answer:
Your answer is potASSium Iodide
Explanation:
I took the test yesterday
Please give brainliest
Answer:
False
Explanation:
Fossil fuels are used as a source of energy to this day.
The answer is A. You record ,write down, what is happening with the experiment.