Answer:
The calculated volume of a lithium atom is 1.47 X 10⁻²⁹ m³.
Explanation:
Assuming the atom's volume is spherical (though it’s actually more complex), the volume is mathematically represented by:
----------------------------------------------------------------------------------------(Eq. 1)
Here, R corresponds to the lithium atom's radius. Since the radius is provided in picometers, we first convert it into meters.
Substituting this value into Eq.1 provides the desired result.
V= 1.47 X 10⁻²⁹ m³
Analyzing the formula for sulfuric acid reveals the molar proportions:
H: S: O
2: 1: 4
Next, we need to convert the provided mass of hydrogen into moles, calculated by:
Moles = mass / Mr
Moles = 7.27 / 1
Moles = 7.27
Thus, the number of moles for each element are:
S = 7.27 / 2 = 3.64 moles
O = 7.27 * 2 = 14.54 moles
Subsequently, the masses for sulfur and oxygen are:
S = 32 * 3.64 = 116.48 grams
O = 16 * 14.54 = 232.64 grams
The true statement is B. With identical masses for both metals, the final temperature of the two will be more aligned with 498 K rather than 298 K, as iron's specific heat capacity is significantly greater than that of gold's.
Answer:
78.96 g of NaC2H3O2
Explanation:
The following information is provided:
- The solution's volume is 350 mL
- The solution's molarity is 2.75 M
- The molar mass of NaC2H3O2 is 82.04 g/mol
We need to find the mass of the solute:
First, we calculate the number of moles:
Moles = Molarity × Volume
Thus;
Moles of solute = 2.75 M × 0.350 L
= 0.9625 moles
Next, we find the mass:
Mass = Moles × Molar mass
= 0.9625 moles × 82.04 g/mol
= 78.9635 g
= 78.96 g
Therefore, the amount of NaC2H3O2 required is 78.96 g
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.
