Answer:
3 × 10⁴ kJ
Explanation:
Step 1: Write the balanced thermochemical equation
C₃H₈(g) + 5 O₂(g) ⟶ 3 CO₂(g) + 4 H₂O(g) ΔH = -2220 kJ
Step 2: Calculate the moles corresponding to 865.9 g of H₂O
The molar mass of H₂O is 18.02 g/mol.
865.9 g × 1 mol/18.02 g = 48.05 mol
Step 3: Calculate the heat produced when 48.05 moles of H₂O are produced
According to the thermochemical equation, 2220 kJ of heat are evolved when 4 moles of H₂O are produced.
48.05 mol × 2220 kJ/4 mol = 2.667 × 10⁴ kJ ≈ 3 × 10⁴ kJ
1 tablespoon = 0.5 ounces
We are required to find for 2 table spoons.
2 table spoons = 2 x 0.5 = 1 ounce.
Each bottle has 16 ounce.
Number of bottles = 4
So total number = 4 x 16 = 64 ounces.
Number of 2 table spoons =
= 64
Thus there are 64 2-tablespoon doses are in 4 bottles of medication containing 16 ounces each.
The nuclear reactions which are under experimenter's control are said to be controlled nuclear reactions. In this, you can maintain the speed of the incident particle. α and β-decay process are examples of non-controlled nuclear reactions.
Explanation:
Supersaturation occurs with a chemical solution when the concentration of a solute exceeds the concentration specified by the value equilibrium solubility. Most commonly the term is applied to a solution of a solid in a liquid.
Answer:
The answer to your question is AgCl
Explanation:
Data
Silver = Ag = 75%
Chlorine = Cl = 25%
1.- Convert percent numbers to grams
Silver = 75 g
Chlorine = 25 g
2.- Calculate the moles of each element
Mass number Ag = 108 g
Mass number Cl = 35.5 g
108 g of Ag ------------------ 1 mol
75 g of Ag ------------------ x
x = (75 x 1) / 108
x = 75 / 108
x = 0.69 moles
35.5 g of Cl ------------------ 1 mol
25 g of Cl ----------------- x
x = (25 x 1) / 35.5
x = 0.70 moles
3.- Divide by the lowest number of moles
Ag = 0.69/0.69 = 1
Cl = 0.70 / 0.69 = 1.02 ≈ 1
4.- Write the empirical formula
Ag₁ Cl₁ = AgCl