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.
The solution to your inquiry is: c = a + b - d. In the chemical equation aA + bB → cC + dD, c may take any value from 1 to however many are needed for the equation to maintain its balance. For instance, if we consider c + d = a + b, we can express c as a + b - d. If we assign values a = 1; b = 3, and d = 2, then c equals 1 + 3 - 2, resulting in c = 2, and so forth.
Answer:
The heat capacity of the calorimeter is 
= 54.4 
Explanation:
Given the data
Heat supplied Q = 4.168 KJ = 4168 J
Mass of water 
= 75.40 gm
Change in temperature = ΔT = 35.82 - 24.58 = 11.24 °C
From the conditions provided
Q = 
ΔT + ΔT
Plugging all values into the above equation yields
4168 = 75.70 × 4.18 × 11.24 + × 11.24
611.37 = × 11.24
= 54.4
This represents the heat capacity of the calorimeter.
The new pressure of the gas is calculated to be 40.7 kPa. Using the principle that P1 • V1 = P2 • V2, we can set 98.8 kPa (P1) multiplied by 21.7 mL (V1) equal to P2 (unknown pressure) multiplied by 52.7 mL (V2). To isolate P2, we rearrange the equation to P2 = (98.8 kPa • 21.7 mL) / 52.7 mL, resulting in P2 equal to 40.7 kPa.
The question appears to be confusing. The periodic table consists of elements organized by increasing atomic number.
