Aqueous solutions of copper (II) bromide and silver (1) acetate react to form solid
1 answer:
Answer:
5.63 g
Explanation:
Step 1: Write the balanced equation
CuBr₂(aq) + 2 AgCH₃CO₂(aq) ⇒ 2 AgBr(s) + Cu(CH₃CO₂)₂(aq)
Step 2: Calculate the reacting moles of copper (II) bromide
30.0 mL of 0.499 M CuBr₂ react. The reacting moles of CuBr₂ are:
Step 3: Calculate the moles formed of silver (I) bromide
The molar ratio of CuBr₂ to AgBr is 1:2. The moles formed of AgBr are 2/1 × 0.0150 mol = 0.0300 mol.
Step 4: Calculate the mass corresponding to 0.0300 mol of AgBr
The molar mass of AgBr is 187.77 g/mol.
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Answer: The empirical formula for the given compound is
Explanation:
The chemical equation for the combustion of compound having carbon and hydrogen follows:
where, 'x' and 'y' are the subscripts of carbon and hydrogen respectively.
We are given:
Mass of
We know that:
Molar mass of carbon dioxide = 44 g/mol
For calculating the mass of carbon:
In 44 g of carbon dioxide, 12 g of carbon is contained.
So, in 22.0 g of carbon dioxide, of carbon will be contained.
For calculating the mass of hydrogen:
Mass of hydrogen = Mass of sample - Mass of carbon
Mass of hydrogen = 7.0 g - 6 g
Mass of hydrogen = 1.0 g
To formulate the empirical formula, we need to follow some steps:
Step 1: Converting the given masses into moles.
Moles of Carbon =
Moles of Hydrogen =
Step 2: Calculating the mole ratio of the given elements.
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.5 moles.
For Carbon =
For Hydrogen =
Step 3: Taking the mole ratio as their subscripts.
The ratio of Fe : C : H = 1 : 2
Hence, the empirical formula for the given compound is