A piece of wood near a fire is at 23°C. It gains 1,160 joules of heat from the fire and reaches a temperature of 42°C. The speci
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Answer:
Two non bonded electron pairs and four bonded electron pairs
Explanation:
An image of the compound as obtained from chemlibretext is attached to this answer.
The ion ICl4- ion, is an AX4E2 ion. This implies that there are four bond pairs and two lone pairs of electrons. As expected, the shape of the ion is square planar since the lone pairs are found above and below the plane of the square. This is clear from the image attached.
<h3>Answer:</h3>
87.40 %
<h3>Explanation:</h3>Concept being tested: Percent yield of a product
We are given;
Mass of Sodium oxide 5 g
Experimental or Actual yield of sodium peroxide IS 5.5 g
We are required to calculate the percent yield of sodium peroxide;
The equation for the reaction that forms sodium peroxide is
2Na₂O + O₂ → 2Na₂O₂
<h3>Step 1; moles of sodium oxide</h3>Moles = mass ÷ molar mass
Molar mass of sodium oxide is 61.98 g/mol
Therefore;
Moles = 5 g ÷ 61.98 g/mol
= 0.0807 moles
<h3>Step 2: Theoretical moles of sodium peroxide produced </h3>From the equation, 2 moles of sodium oxide produces 1 mole of sodium peroxide.
Thus, moles of sodium peroxide used is 0.0807 moles
<h3>Step 3: Theoretical mass of sodium peroxide used</h3>Mass = Number of moles × Molar mass
Molar mass of sodium peroxide = 77.98 g/mol
Therefore;
Theoretical mass = 0.0807 moles × 77.98 g/mol
= 6.293 g
Theoretical mass of Na₂O₂ is 6.293 g
<h3>Step 4: Percent yield of Na₂O₂</h3>- We know that percent yield is given by the ratio of actual yield to theoretical yield expressed as a percentage.
= 87.40 %
Therefore, the percentage yield of sodium peroxide is 87.4%