C.<span>Wave A will have a louder sound than wave B
</span>
Answer:
Melting Is when a substance is actually melting and melting point is a point at which a substance is able to melt.
Answer:
When an element loses an electron, its oxidation number increases.
Explanation:
The oxidation number of an element indicates the hypothetical charge of an atom in a compound. It is hypothetical because, in the context of a compound, the elements may not necessarily be ionic. When the number of electrons associated with an atom changes, its oxidation number also changes. When an element loses an electron, its oxidation number increases.
Answer:
<em />
<em>a) Balanced chemical equation:</em>
<em />
<em> </em><em />
<em />
<em>b) Theoretical yield:</em>
c) % yield:
Explanation:
The complete question is:
<em>In a particular reaction 6.80g of dinitrogen trioxide gas (N₂0₃) was actually produced by reacting 8.75g of oxygen gas (O₂) with excess nitrogen gas (N₂)</em>
<em>a) Write a balanced chemical equation for the reaction. Be sure to include physical states in the equation.</em>
<em>b) Calculate the theoretical yield (in grams) of dinitrogen trioxide: Use dimensional analysis</em>
<em>c) Calculate the % yield of the product</em>
<em />
<h2>Solution</h2>
<em />
<em>a) Write a balanced chemical equation for the reaction. Be sure to include physical states in the equation.</em>
<em />
<em> </em><em />
<em />
Check the balance:
<em />
Atom Left-handside Right-hand side
N 2×2=4 2×2=4
O 3×2=6 2×3=6
- Mole ratio: it is the ratio of the coefficients of the balanced equation
<em>b) Calculate the theoretical yield (in grams) of dinitrogen trioxide: Use dimensional analysis</em>
<em />
<u>1. Convert 8.75 g of O₂(g) to number of moles</u>
- number of moles = mass in grams / molar mass
- molar mass of O₂ = 15.999g/mol
- number of moles = 8.75g / 15.999 g/mol = 0.5469 mol O₂
<u />
<u>2. Use dimensional analysis to calculate the maximum number of moles of N₂O₃(g) that can be produced</u>
<u>3. Convert to mass in grams</u>
- mass = number of moles × molar mass
- molar mass of N₂O3 = 76.01g/mol
- mass = 0.3646mol × 76.01g/mol = 27.7g N₂O3
<em>c) Calculate the % yield of the product</em>
<em />
Formula:
<em />
- %yield = (actual yield/theoretical yield)×100
Substitute and compute:
- % yield = (6.80g/27.7g)×100 = 24.5%
<em />
Answer:
The molarity of the HCl solution is 4M.
Explanation:
Hence, the molarity of the HCl solution = 4 M