<em><u>look at the clues by it and try not to trust the links they trying to give u...</u></em>
<em><u>but i kinda dont know myself any periodic table i can look at?</u></em>
Answer:
0.7561 g.
Explanation:
- The hydrogen than can be prepared from Al according to the balanced equation:
<em>2Al + 6HCl → 2AlCl₃ + 3H₂,</em>
It is clear that 2.0 moles of Al react with 6.0 mole of HCl to produce 2.0 moles of AlCl₃ and 3.0 mole of H₂.
- Firstly, we need to calculate the no. of moles of (6.8 g) of Al:
no. of moles of Al = mass/atomic mass = (6.8 g)/(26.98 g/mol) = 0.252 mol.
<em>Using cross multiplication:</em>
2.0 mol of Al produce → 3.0 mol of H₂, from stichiometry.
0.252 mol of Al need to react → ??? mol of H₂.
∴ the no. of moles of H₂ that can be prepared from 6.80 g of aluminum = (3.0 mol)(0.252 mol)/(2.0 mol) = 0.3781 mol.
- Now, we can get the mass of H₂ that can be prepared from 6.80 g of aluminum:
mass of H₂ = (no. of moles)(molar mass) = (0.3781 mol)(2.0 g/mol) = 0.7561 g.
Answer:
The Supreme Court of Appeal
Explanation:
The Supreme Court of Appeal is based in Bloemfontein in the Free State. Except for the Constitutional Court, it is the highest court in South Africa and it only deals with cases sent to it from the High Court.
To solve this given problem, we can use the equation below:
ΔG=ΔH - T*ΔS
We are information and values are given and can be used in solving the ΔG of this particular reaction.
ΔH=-99.84kJ
ΔS=-16.80 J/K
T=298K
ΔG=(-99.84kJ)-(298K*-16.80J/K)
ΔG=-94.83kJ
The answer for ΔG is -94.83kJ.
Answer:
B)
an atom of mercury has a different mass than an atom of copper.
Explanation:
