<h2>
Answer:</h2>
6 × 10²⁴ molecules F₂
<h2>
General Formulas and Concepts:</h2><h3><u>Chemistry</u></h3>
<u>Atomic Structure</u>
- Using Dimensional Analysis
- Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.
<h3><u>Math</u></h3>
<u>Pre-Algebra</u>
Order of Operations: BPEMDAS
- Brackets
- Parenthesis
- Exponents
- Multiplication
- Division
- Addition
- Subtraction
<h2>
Explanation:</h2>
<u>Step 1: Define</u>
10 mol F₂
<u>Step 2: Identify Conversions</u>
Avogadro's Number
<u>Step 3: Convert</u>
<u />
= 6.022 × 10²⁴ molecules F₂
<u>Step 4: Check</u>
<em>We are given 1 sig fig. Follow sig fig rules and round.</em>
6.022 × 10²⁴ molecules F₂ ≈ 6 × 10²⁴ molecules F₂
Concentration of solution: C=n/v
=> C=5mol/10L = 0.5mol/L
What do u mean P=? What is P?
Answer:
1040%
Explanation:
To solve this question we must convert the mass of Iron to moles in order to find limiting reactant. With limiting reactant we can find the theoretical moles of hydrogen and theoretical mass:
Percent yield = Actual yield (5.40g) / Theoretical yield * 100
<em>Moles Fe -Molar mass: 55.845g/mol-:</em>
10.3g * (1mol / 55.845g) = 0.184 moles of Fe will react.
For a complete reaction of these moles there are necessaries:
0.184 moles Fe* ( 3 mol H2SO4 / 2 mol Fe) = 0.277 moles H2SO4.
As there are 14.8 moles of the acid, <em>Fe is limiting reasctant.</em>
The moles of H2 produced are:
0.184 moles Fe* ( 3 mol H2 / 2 mol Fe) = 0.277 moles H2
The mass is:
0.277 moles H2 * (2.016g/mol) = 0.558g H2
Percent yield is:
5.40g / 0.558g * 100 = 1040%
It is possible the experiment wasn't performed correctly
Answer:
174.259 g/mol
Explanation:
The molecular weight of potassium (K2so4) is 174.259 g/mol .
<em>Hope </em><em>it </em><em>is </em><em>helpful</em><em> to</em><em> you</em>
