Answer:
Mass = 17.12 g
Explanation:
Given data:
Mass of Al = 3.90 g
Mass of H₂SO₄ = 13.65
Mass of aluminium sulfate = ?
Solution:
Chemical equation:
3H₂SO₄ + 2Al → Al₂(SO₄)₃ + 3H₂
Now we will calculate the number of moles of each reactant.
Moles of H₂SO₄:
Number of moles = mass/ molar mass
Number of moles = 13.65 g/ 98.079 g/mol
Number of moles = 0.14 mol
Moles of Al:
Number of moles = mass/ molar mass
Number of moles = 3.90 g/ 27 g/mol
Number of moles = 0.14 mol
Now we will compare the moles of aluminium sulfate with sulfuric acid and aluminium.
H₂SO₄ : Al₂(SO₄)₃
3 : 1
0.14 : 1/3×0.14 = 0.05
Al : Al₂(SO₄)₃
2 : 1
0.14 : 1/2×0.14 = 0.07
The number of moles of aluminium sulfate produced by sulfuric acid are less so it will limiting reactant and limit the amount of aluminium sulfate.
Mass of aluminium sulfate:
Mass = number of moles × molar mass
Mass = 0.05 mol × 342.15 g/mol
Mass = 17.12 g
Tides would be much weaker. Tidal forces from the moon would be eight times weaker.
Answer:
75603.86473 K
Explanation:
Given that:
The 1st excited electronic energy level of He atom = 3.13 × 10⁻¹⁸ J
The objective of this question is to estimate the temperature at which the ratio of the population will be 5.0 between the first excited state to the ground state.
The formula for estimating the ratio of population in 1st excited state to the ground state can be computed as:
From the above equation:
Δ E = energy difference = 3.13 × 10⁻¹⁸ J
k = Boltzmann constant = 1.38 × 10⁻²³ J/K
Thus:
T = 75603.86473 K
Answer:
A team of Chinese researchers have turned cheap copper into a new material “almost identical” to gold, according to a study published in peer-reviewed journal Science Advances on Saturday. The fast-moving ionized particles blasted copper atoms off the target.
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Explanation:
