Here we will use the general formula of Nernst equation:
Ecell = E°Cell - [(RT/nF)] *㏑Q
when E cell is cell potential at non - standard state conditions
E°Cell is standard state cell potential = - 0.87 V
and R is a constant = 8.314 J/mol K
and T is the temperature in Kelvin = 73 + 273 = 346 K
and F is Faraday's constant = 96485 C/mole
and n is the number of moles of electron transferred in the reaction=2
and Q is the reaction quotient for the reaction
SO42-2(aq) + 4H+(aq) +2Br-(aq) ↔ Br2(aq) + SO2(g) +2H2O(l)
so by substitution :
0 = -0.87 - [(8.314*346K)/(2* 96485)*㏑Q → solve for Q
∴ Q = 4.5 x 10^-26
Al(s) + 2AgNO3(aq) = Al(NO3)3(aq) + 3 Ag (s)
is a single replacement reaction
A single replacement reaction is a type of chemical reaction were element react with a compound and the element take place of another element in that compound. In the reaction above Aluminium (Al) take the place of silver (Ag) from it compound.that is AgNO3. single replacement reaction is possible because aluminium is in high in reactivity series as compared to silver.
Answer:
0.11 mol
Explanation:
<em>This is the chemical formula for acetic acid (the chemical that gives the sharp taste to vinegar): CH₃CO₂H. An analytical chemist has determined by measurements that there are 0.054 moles of oxygen in a sample of acetic acid. How many moles of hydrogen are in the sample?</em>
Step 1: Given data
- Formula of acetic acid: CH₃CO₂H
- Moles of oxygen in the sample of acetic acid: 0.054 moles
Step 2: Establish the appropriate molar ratio
According to the chemical formula of acetic acid, the molar ratio of H to O is 4:2.
Step 3: Calculate the moles of atoms of hydrogen
We will use the theoretical molar ratio for acetic acid.
0.054 mol O × (4 mol H/2 mol O) = 0.11 mol H
Answer:
Explanation:
Here we have the mass of CO₂ added = 340 g
From
We have, where the molar mass of CO₂ is 44.01 g/mol
Therefore,
71. Included drawing attached
72. Here we have the pressure of the gas given by Charles law which can be resented as follows;
Where:
P₁ = Initial pressure = 6.1 atmospheres
P₂ = Final pressure
T₁ = Initial Temperature = 293 K
T₂ = Initial Temperature = 313 K
Therefore,
The molar mass of anhydrous Na₂SO₄ = [2(23) + 32 + 4(16)]
= 142 g/mol
If the molar mass of hydrated Na₂SO₄ = 322 g/mol
Since hydrated salt = Anhydrous Salt + Water
Then the mass of hydration (Water)= 322 g/mol - 142 g/mol
= 180 g/mol
Since the molar mass of water itself is 18 g/mol
⇒ Moles of water = 180 g/mol ÷ 18g/mol
= 10
Thus n = 10; the formula of the hydrated salt is Na₂SO₄ · 10H₂O (Sodium Sulphate Decahydrate)
