Answer:
The specific heat value for silver is 0.236 J/g-C.
Explanation:
Silver has a mass of 25 grams.
The temperature shifts from 31.5° C to 58.7° C.
The required heat is equivalent to 25 g.
To determine silver's specific heat, the following equation applies:
Where c represents the specific heat of silver.
Thus, the specific heat of silver is 0.236 J/g-C.
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.
<span>4.3065 g
To begin with, consult the atomic masses for each involved element.
Atomic weight of Calcium = 40.078
Atomic weight of Carbon = 12.0107
Atomic weight of Hydrogen = 1.00794
Atomic weight of Oxygen = 15.999
Atomic weight of Sulfur = 32.065
Next, compute the molar masses of both reactants and the product.
Molar mass H2SO4 = 2 * 1.00794 + 32.065 + 4 * 15.999
= 98.07688 g/mol
Molar mass CaCO3 = 40.078 + 12.0107 + 3 * 15.999
= 100.0857 g/mol
Molar mass CaSO4 = 40.078 + 32.065 + 4 * 15.999
= 136.139 g/mol
The balanced equation for the reaction between H2SO4 and CaCO3 is:
CaCO3 + H2SO4 ==> CaSO4 + H2O + CO2
Thus, 1 mole each of CaCO3 and H2SO4 is necessary to generate 1 mole of CaSO4. Let's check the amount of moles we have for CaCO3 and H2SO4.
CaCO3: 3.1660 g / 100.0857 g/mol = 0.031632891 mol
H2SO4: 3.2900 g / 98.07688 g/mol = 0.033545113 mol
H2SO4 is in slight excess, therefore CaCO3 is the limiting reactant, suggesting we can expect 0.031632891 moles of product. To find the mass, multiply the number of moles by the molar mass calculated previously.
0.031632891 mol * 136.139 g/mol = 4.306470148 g
Given that we have 5 significant figures from our data, we round the final result to 5 figures, yielding 4.3065 g</span>
Answer:NH₃/NH₄Cl
Explanation:
The pH of a buffer can be determined using Henderson-Hasselbalch's equation.
![pH=pKa+log\frac{[base]}{[acid]}](https://tex.z-dn.net/?f=pH%3DpKa%2Blog%5Cfrac%7B%5Bbase%5D%7D%7B%5Bacid%5D%7D)
When the concentration of acid equals that of the base, the pH aligns with the pKa of the buffer. The ideal pH range is pKa ± 1.
Below are the buffers and their corresponding pKa values:
- CH₃COONa/CH3COOH (pKa = 4.74)
Thus, the ideal buffer is NH₃/NH₄Cl.
The proportion of component A by mass for substance AB is given by 75%.
Further explanation
According to Proust's Comparative Law, compounds are made from elements that maintain the same Mass Comparison, ensuring that compounds have a consistent ratio of elements.
The empirical formula presents the mole ratio of elements forming a compound.
In the case of substance AB₂, 60.0% of its mass is attributed to A.
For instance, if the mass of AB₂ is 100 grams, then the mass of A would be 60 grams, and the mass of B would be 40 grams, divided according to the coefficient in compound AB₂ which is 2, leading to 20 grams.
Thus, for compound AB, the total mass is the sum of mass A and mass B, which equals 60 grams plus 20 grams, resulting in a total mass of 80 grams.
Consequently, the percentage of compound A calculates to (60: 80) = 75%.
