0.012 mol of CO₂ can be produced from 3.50 g of baking powder.
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What is baking powder?</h3>
- Baking powder is a dry chemical leavener composed of carbonate or bicarbonate and a weak acid.
- The addition of a buffer, such as cornstarch, prevents the base and acid from reacting prematurely.
- Baking powder is used in baked goods to increase volume and lighten the texture.
To find how many moles of CO₂ are produced from 1.00 g of baking powder:
The balanced equation is:
- Ca(H₂PO₄)₂(s) + 2NaHCO₃(s) → 2CO₂(g) + 2H₂O(g) + CaHPO₄(s) + Na₂HPO₄(s)
On 3.50 g of baking power:
- mCa(H₂PO₄)₂ = 0.35 × 3.50 = 1.225 g
- mNaHCO₃ = 0.31 × 3.50 = 1.085 g
The molar masses are: Ca = 40 g/mol; H = 1 g/mol; P = 31 g/mol; O = 16 g/mol; Na = 23 g/mol; C = 12 g/mol.
So,
- Ca(H₂PO₄)₂: 40 + 4 × 1 + 31 + 8 × 16 = 203 g/mol
- NaHCO₃: 23 + 1 + 12 + 3 × 16 = 84 g/mol
The number of moles is the mass divided by molar mass, so:
- nCa(H₂PO₄)₂ = 1.225/203 = 0.006 mol
- nNaHCO₃ = 1.085/84 = 0.0129 mol
First, let's find which reactant is limiting.
Testing for Ca(H₂PO₄)₂, the stoichiometry is:
- 1 mol of Ca(H₂PO₄)₂ ---------- 2 mol of NaHCO₃
- 0.006 of Ca(H₂PO₄)₂ -------- x
By a simple direct three rule:
So, NaHCO₃ is in excess.
The stoichiometry calculus must be done with the limiting reactant, then:
- 1 mol of Ca(H₂PO₄)₂ ------------- 2 mol of CO₂
- 0.006 of Ca(H₂PO₄)₂ -------- x
By a simple direct three rule:
Therefore, 0.012 mol of CO₂ can be produced from 3.50 g of baking powder.
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The correct question is given below:
Calcium dihydrogen phosphate, Ca(H2PO4)2, and sodium hydrogen carbonate, NaHCO3, are ingredients of baking powder that react with each other to produce CO2, which causes dough or batter to rise: Ca(H2PO4)2(s) + NaHCO3(s) → CO2(g) + H2O(g) + CaHPO4(s) + Na2HPO4(s)[unbalanced] If the baking powder contains 31.0% NaHCO3 and 35.0% Ca(H2PO4)2 by mass: (a) How many moles of CO2 are produced from 3.50 g of baking powder?
