Answer:
The equilibrium constant Ksp of the generic salt AB2 = 6.4777 *10^-8 M
Explanation:
Step 1: The balanced equation
AB2 ⇒ A2+ + 2B-
Step 2: Given data
Concentration of A2+ = 0.00253 M
Concentration of B- = 0.00506 M
Step 3: Calculate the equilibrium constant
Equilibrium constant Ksp of [AB2] = [A2+][B-]²
Ksp = 0.00253 * 0.00506² = 6.4777 *10^-8 M
The equilibrium constant Ksp of the generic salt AB2 = 6.4777 *10^-8 M
Answer:
167,3 grams of O2 (g)
Explanation:
According to the following balanced equation:
C3H8 + 5 02 ---> 3 CO2 + 4 H20
We calculate the mass of the moles:
5 mol O2 = 16grams/mol x2x 5= 160 grams/mol
1 mol C3H8= 3 x12 grams/mol + 8 x 1 gram/mol= 44 grams/mol
If 44 grams C3H8 react with--------- 160 grams O2
46 gramsC3H8 react with --------X = (46x160)/44 =167, 3 grams O2
Answer:
2CO + O₂ → 2CO₂ ΔH = -566 kj
Explanation:
Given data:
Energy evolved when 1 mole of CO react = 283 Kj
Energy evolved when 2 mole of CO react = ?
Solution:
Chemical equation:
2CO + O₂ → 2CO₂
It is given when one mole of CO react with oxygen 283 KJ energy is produced.
When 2 mole react,
2 ×-283 kj = -566 kj
Thermal equation:
2CO + O₂ → 2CO₂ ΔH = -566 kj
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Answer:
3.25 mol CO₂
Explanation:
Step 1: Write the balanced equation
C(s) + O₂(g) ⇒ CO₂(g)
Step 2: Establish the appropriate molar ratio
According to the balanced equation, the molar ratio of O₂ to CO₂ is 1:1.
Step 3: Calculate the number of moles of CO₂ produced from 3.25 moles of O₂
We will use the previously established molar ratio.
3.25 mol O₂ × 1 mol CO₂/ 1 mol O₂ = 3.25 mol CO₂
