Answer:
Explanation:
A mole is defined as the number of molecules divided by 6.02×10^23
Mole = (2×10^19)/(6.02×10^23)
Mole = 3.32×10^-5 mole
Answer:
The accurate answer is 596.5 kJ.
Explanation:
The question specifies that the mass of ethanol, C2H5OH, is 20 grams.
The molar mass of ethanol is 46 g/mol.
To find the moles of ethanol, we use the formula:
n = mass / molar mass
= 20/46 = 0.435 moles
According to the question, the standard heat of combustion for ethanol is 1372 kJ/mol. Hence, one mole releases 1372 kilojoules during combustion.
The energy produced from burning 20 grams of ethanol completely is 0.435 * 1372 = 596.5 kJ.
Response:
9.606 g
Clarification:
Step 1: Write the balanced combustion equation
C₂H₆O(l) + 3 O₂(g) → 2 CO₂(g) + 3 H₂O(g)
Step 2: Determine the moles for 11.27 g of H₂O
The molar mass of H₂O is 18.02 g/mol.
11.27 g × (1 mol/18.02 g) = 0.6254 mol
Step 3: Find the moles of C₂H₆O that produced 0.6254 moles of H₂O
The ratio of C₂H₆O to H₂O is 1:3. Thus, the moles of C₂H₆O are 1/3 × 0.6254 mol = 0.2085 mol
Step 4: Calculate the mass for 0.2085 moles of C₂H₆O
The molar mass of C₂H₆O is 46.07 g/mol.
0.2085 mol × 46.07 g/mol = 9.606 g
Cu(NO3)2 --> MM187.5558
NiNO3 *COEF2* --> 120.6983
Different wavelengths are involved.
Explanation:
When magnesium ignites with a bright white flame, it indicates that various wavelengths are related to the electron transitions occurring in the magnesium atom.
- Upon combustion, the electrons within the atom become excited.
- They emit characteristic light that corresponds to their energy levels.
- White light consists of a mix of different wavelengths.
- Seeing white light implies that multiple wavelengths combined are responsible for the observed emission.
Learn more:
Spectrum
