Answer:
25.2 kJ
Explanation:
The full question can be found in the image linked to this response.
It's important to highlight that the heat absorbed by the 2.00 L of water for increasing its temperature from the beginning to the end comes solely from the burning of benzoic acid, as there are no heat transfers to the container or the surroundings.
To find the heat released from benzoic acid combustion, we simply measure the heat needed to warm the water.
Q = mCΔT
To find the mass of the water,
Density = (mass)/(volume)
Mass = Density × volume
Density = 1 g/mL
Volume = 2.00 L = 2000 mL
Mass = 1 × 2000 = 2000 g
C = specific heat of water = 4.2 J/g.°C
ΔT = (final temperature) - (Initial temperature)
<pAccording to the graph,
Final water temperature = 25°C
Initial water temperature = 22°C
ΔT = 25 - 22 = 3°C
Q = (2000×4.2×3) = 25,200 J = 25.2 kJ
Hope this Helps!!!
Answer:
Oxygen's mass percent in Fe(OH)3 is 44.92%
Explanation: The mass percentage is a means of indicating the concentration of a specific element within a compound. It is determined through the ratio of the element's mass to the compound's total mass, multiplied by 100.
•First calculate the overall mass of the compound
•Fe's molar mass = 55.85 g/mol
•O's molar mass = 16 g/mol
•H's molar mass = 1 g/mol
Using these values, we can compute the molecular mass of Fe(OH)3 = 55.85 g/mol + (16 g/mol)3 + (1 g/mol)3
=55.85 g/mol + 48 g/mol + 3 g/mol
=106.85 g/mol
Mass percent of an element = mass of element/total mass of compound × 100
In the case of 3 oxygen atoms present within the compound, the mass of oxygen totals 48 g/mol
Mass percent of oxygen= 48 g/mol/106.85 g/mol × 100
= 0.4492×100= 44.92%
[[TAG_31]]Thus, the mass percent of oxygen in Fe(OH)3 amounts to 44.92%[[TAG_32]]
Vapor pressure refers to the force exerted by vapor or gas molecules above the surface of a liquid. It is inversely related to the concentration of solute particles; an increase in solute concentration results in a decrease in vapor pressure, and vice versa. For (a), it dissociates into two particles. In (b), the total count of particles from dissociation becomes 1 + 2, totaling three. For (c), dissociation yields 1 + 3 for a total of four particles. (d) Since sucrose is a covalent compound, it does not break apart into ions, so it remains as one particle. For (e), dissociation results in 1 + 1, equating to two particles.
The stated condition has been verified. Construct the resonance structure for CSO, where the central atom carries a +2 formal charge and the oxygen atom has a +1 charge. We need to create the resonance structure for CSO as shown in the figure. According to the problem, there is a +2 formal charge on the central atom and a +1 charge on the oxygen atom. The central atom in this structure is sulfur. We will calculate the formal charge of sulfur based on the information presented, demonstrating that it aligns with the necessary formal charges.
Response:
H₂SO₄
Clarification:
Given a compound consisting of 0.475 g H, 7.557 g S, and 15.107 g O, we must compute the empirical formula by following specific steps.
Step 1: Compute the total mass of the compound
Total mass = mass H + mass S + mass O = 0.475 g + 7.557 g + 15.107 g
Total mass = 23.139 g
Step 2: Determine the percentage composition.
H: (0.475g/23.139g) × 100% = 2.05%
S: (7.557g/23.139g) × 100% = 32.66%
O: (15.107g/23.139g) × 100% = 65.29%
Step 3: Divide each percentage by the element's atomic mass
H: 2.05/1.01 = 2.03
S: 32.66/32.07 = 1.018
O: 65.29/16.00 = 4.081
Step 4: Normalize all values by the smallest one
H: 2.03/1.018 ≈ 2
S: 1.018/1.018 = 1
O: 4.081/1.018 ≈ 4
Thus, the empirical formula for the compound is H₂SO₄.
