Thomson's model of the atom was called the plum pudding model. He discovered electrons, so he placed them in the atoms. This was before the nucleus was discovered.
Now, the current model is an atom that contains a positively charged nucleus (with both protons and neutrons), and negatively charged orbitals with electrons.
The molar mass of the compound is 68 g/mol.
<h3>What is the molar mass?</h3>
The Osmotic pressure can be obtained from the relationship;
π= iCRT
π= osmotic pressure = 28.1 mmHg or 0.037 atm
i = Vant Hoff factor = 1
C = concentration = ?
R = gas constant = 0.082 atmLK-1Mol
T = temperature = 20°c + 273 = 293 K
C = π/iRT
C = 0.037/1 * 0.082 * 293
C = 0.0015 M
Now;
Number of moles = C/V = 0.0015/100 * 10^-3
= 0.015 moles
Number of moles = mass/molar mass
Molar mass = mass/Number of moles = 0. 102 g/ 0.015 moles = 68 g/mol
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Enthalpy change = mass * specific heat capacity * temperature change
Mass is 25.0 (given)
Specific heat capacity is 2.108 (checked online)
Temperature change : none
So input these into the equation :
25.0 * 2.108 = 52.7
Answer:
151.87dm³
Explanation:
Given parameters:
Volume of hydrogen gas = 6.78mole
Unknown:
Volume of hydrogen gas formed at STP = ?
Solution:
To solve this problem;
1 mole of a gas at STP = 22.4dm³ So;
6.78 mole of gas = 6.78 x 22.4 = 151.87dm³
Answer:
10 g H₂SO₄
General Formulas and Concepts:
<u>Chemistry - Stoichiometry</u>
- Reading a Periodic Table
- Using Dimensional Analysis
Explanation:
<u>Step 1: Define</u>
Given: 8 g SO₃
RxN: SO₃ + H₂O → H₂SO₄
<u>Step 2: Identify Conversions</u>
Molar Mass of S - 32.07 g/mol
Molar Mass of O - 16.00 g/mol
Molar Mass of H - 1.01 g/mol
Molar Mass of SO₃ - 32.07 + 3(16.00) = 80.07 g/mol
Molar mass of H₂SO₄ - 2(1.01) + 32.07 + 4(16.00) = 98.09 g/mol
<u>Step 3: Stoichiometry</u>
<u />
= 9.80042 g H₂SO₄
<u>Step 4: Check</u>
<em>We are given 1 sig fig. Follow sig fig rules and round.</em>
9.80042 g H₂SO₄ ≈ 10 g H₂SO₄
