A water molecule contains an oxygen atom and two hydrogen atoms which are covalently bonded to the oxygen atom.Atoms in a covalently bonded molecule are always fighting for the shared electrons, the atoms attraction to the shared electrons is called the electronegativity. Therefore, the more electronegative an atom is the more it attracts the shared electrons.The force of attraction between a partially electronegative atom and another partially positive atom is the hydrogen bond. It is the hydrogen bond that pulls water molecules together which results into a cohesive force between the water molecules.
Answer:
The answer for the first problem is: C₆N₁H₁₁O₁ or C₆NH₁₁O
Explanation:
Nylon composition: Mass Divide by the atomic mass
Carbon 63.68 % 63.68 g 63.68/ 12 = 5.3
Nitrogen 12.38 % 12.38 g 12.38/14 = 0.88
Hydrogen 9.8% 9.8 g 9.8/1 = 9.8
Oxygen 14.14% 14.14 g 14.14/16 = 0.88
We choose the lowest number that is 0.88 for nitrogen and oxygen and divide the four results by this number
Carbon 5.3/0.88 = 6
Nitrogen 0.88/0.88 = 1
Hydrogen 9.8/0.88 = 11.1 = 11
Oxygen 0.88/ 0.88 = 1
Then the empirical formula has this coefficients
C₆N₁H₁₁O₁ or C₆NH₁₁O
Answer:
∇T = 51.68°C
Explanation:
Mass = 150g
Heat Energy (Q) = 1.0*10³J
Change in temperature ∇T = ?
Q = mc∇T
Q = heat energy
M = mass
C = specific heat capacity of the gold = 0.129j/g°C
∇T = change in temperature
Q = Mc∇T
1.0*10³ = 150 * 0.129 * ∇T
1000 = 19.35∇T
Solve for ∇T
∇T = 1000 / 19.35
∇T = 51.679°C = 51.68°C
The change in temperature of gold was 51.68°C
Answer:
0.05 mL
Explanation:
Initially, we have a concentrated solution of NaOH, to which we will add water to get a dilute one. To calculate the volume of the initial solution that we have to measure, we can use the dilution rule:
C₁ × V₁ = C₂ × V₂
where,
C₁ is the initial concentration (50% w/w; ρ = 1.52 g/mL)
V₁ is the initial volume
C₂ is the final concentration (0.1 M)
V₂ is the final volume (10 mL)
First, we have to calculate the weight/volume percentage and then the molarity of the first solution.
Now, we can apply the dilution rule.