mass Hydrogen=9.376 g
<h3>Further explanation
</h3>
Reaction
2H₂+O₂⇒2H₂O
mass H₂ = 10 g
mol H₂(MW=2 g/mol) :
10 : 2 = 5
mass O₂=5 g
mol O₂(MW=32 g/mol) :
5 : 32 = 0.156
O₂ limiting reactant
mol H₂: mol O₂ = 2: 1, so mol H₂ :
2 x 0.156 = 0.312
mol H₂ :
5 - 0.132 =4.688
mass of H₂ :
4.688 x 2 =9.376 g
<h3 />
Answer:
This is math?
Explanation:
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Answer:
a. 102.6g/mol
b. Rb⁺
Explanation:
a. The unknown base, XOH, <em>Where X is the alkali metal</em>, reacts with HCl thus:
XOH + HCl → H₂O + XCl
<em>Where 1 mole of the hydroxide reacts per mole of acid. </em>
Moles of HCl spent to reach the equivalence point are:
17.0mL = 0.017L ₓ (2.50mol / L) = 0.0425moles of HCl
As 1 mole of HCl reacts with 1 mole of base, moles of base are 0.0425 moles.
Molar mass of a compound is the ratio between mass in grams and moles of substance, that is:
4.36g / 0.0425mol =
<h3>102.6g/mol</h3>
b) Molar mass of OH is 17g/mol, thus, the molar mass of the alkali metal is:
102.6g/mol - 17g/mol = 85.6g/mol
The mass of Rb is 85.5g/mol, thus, the identity of the alkali metal is
<h3>Rb⁺</h3>
Answer:
P₂ = 16.6 atm
Explanation:
Given data:
Initial pressure = 13.0 atm
Initial temperature = 20.0°C (20+273 = 293 K)
Final temperature = 102.0°C (102+273 =375 K)
Final pressure = ?
Solution:
According to Gay-Lussac Law,
The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.
Mathematical relationship:
P₁/T₁ = P₂/T₂
Now we will put the values in formula:
13.0 atm / 293 K = P₂/375 K
P₂ = 13.0 atm × 375 K / 293 K
P₂ = 4875 atm. K /293 K
P₂ = 16.6 atm
