Question

In: Chemistry

Be sure to answer all parts. Calcium dihydrogen phosphate, Ca(H2PO4)2, and sodium hydrogen carbonate, NaHCO3, are...

Be sure to answer all parts. 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 9.66 g of baking powder? mol CO2 (b) If 1 mol of CO2 occupies 37.0 L at 350°F (a typical baking temperature), what volume of CO2 is produced from 9.66 g of baking powder?

Solutions

Expert Solution

Answer – We are given, reaction –

Ca(H2PO4)2(s) + 2 NaHCO3(s) ----> 2 CO2(g) + 2 H2O(g) + CaHPO4(s) + Na2HPO4(s)

Mass percent of NaHCO3(s) = 31.0% , mass % of Ca(H2PO4)2(s) = 35.0 %

a) Mass of baking powder = 9.66 g , moles of CO2 =

now we need to calculate the mass of each reactant

mass of NaHCO3(s) = 31.0%*9.66 g / 100 %

                                 = 2.995 g

mass of Ca(H2PO4)2(s) = 35.0 % 9.66 g / 100 %

                                      = 3.381 g

Moles of NaHCO3(s) = 2.995 g / 84.00 g.mol-1

                                   = 0.0356 moles

Moles of Ca(H2PO4)2(s) = 3.381 g / 234.05 g.mol-1

                                       = 0.0144 moles

Now we need to calculate the limiting reactant

Moles of CO2 from Ca(H2PO4)2(s)

We know

1 moles of Ca(H2PO4)2(s) = 2 moles of CO2

So, 0.0144 moles of Ca(H2PO4)2(s) = ?

= 0.0288 moles of CO2

Moles of CO2 from the NaHCO3(s)

1 moles of NaHCO3(s) = 2 moles of CO2

So, 0.0356 moles of NaHCO3(s) = ?

= 0.0356 moles of CO2

So, the lowest moles of the CO2 from the Ca(H2PO4)2(s) , so limiting eactant is Ca(H2PO4)2(s) .

Moles of CO2 = 0.0288 moles

So, 0.0288 moles of CO2 are produced from 9.66 g of baking powder.

b) We are given, 1 moles of CO2 = 37.0 L at 350°F , mass of baking powder = 9.66 g

We already calculated moles of CO2 produced from 9.66 g of baking powder

So,

1 moles of CO2 = 37.0 L

0.0288 moles of CO2 = ?

= 1.07 L

So, 1.07 L volume of CO2 is produced from 9.66 g of baking powder


Related Solutions

Calcium dihydrogen phosphate, Ca(H2PO4)2, and sodium hydrogen carbonate, NaHCO3, are ingredients of baking powder that react...
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 1.41 g of baking powder? b.) If 1 mol of CO2 occupies 37.0 L at 350...
Calcium dihydrogen phosphate, Ca(H2PO4)2, and sodium hydrogen carbonate, NaHCO3, are ingredients of baking powder that react...
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 6.85 gof baking powder? ____mol CO2 (b) If 1 mol of CO2 occupies 37.0 L at 350°F (a typical...
Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to...
Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq) +NaHCO3(aq) →NaCl(aq) +H2O(l) +CO2(g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the...
WRITE BALANCED, IONIC AND NET EQUATION 1) SODIUM CARBONATE ( Na2CO3) + CALCIUM CARBONATE 2) SODIUM...
WRITE BALANCED, IONIC AND NET EQUATION 1) SODIUM CARBONATE ( Na2CO3) + CALCIUM CARBONATE 2) SODIUM PHOSPHATE ( Na3PO4) + CALCIUM CARBONATE 3) CALCIUM NITRATE ( Ca(NO3)2 + CALCIUM CARBONATE
Be sure to answer all parts. Ammonia is produced by the reaction of nitrogen and hydrogen...
Be sure to answer all parts. Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) → 2NH3(g) 1. Calculate the mass of ammonia produced when 30.0 g of nitrogen react with 11.3 g of hydrogen. 2. Which is the excess reactant and how much of it will be left over when the reaction is complete?
SHOW ALL STEP A solution of calcium carbonate is initially supersaturated with Ca++ and CO3= ions,...
SHOW ALL STEP A solution of calcium carbonate is initially supersaturated with Ca++ and CO3= ions, such that the concentration of each is 1.35 x 10-4 mol/L. When equilibrium is finally reached, what is the concentration of calcium ion. Note that if you use the 4-step approach to equilibrium balance shown in class, electro-neutrality need only consider the calcium and carbonate ions, because they are initially in charge balance (i.e. { Ca++}0 = { CO3=}0 and this implies that [Ca++]0...
PLease Answer all parts of the following: a) The recommended daily allowance of calcium for men...
PLease Answer all parts of the following: a) The recommended daily allowance of calcium for men between the ages of 19 to 50 is 1 000 mg Ca. Three multivitamin tablets are analyzed for calcium gravimetrically with the precipitation of calcium cation by oxalate anion. If the mass dry calcium oxalate obtained is 2.0136 g, how many tablets must a man take in a given day to meet the recommended daily allowance? Ca2+(aq) + C2O42−(aq) ==> CaC2O4 (s) b) Aqueous...
Be sure to answer all parts. Find the pH of the equivalence point and the volume...
Be sure to answer all parts. Find the pH of the equivalence point and the volume (mL) of 0.0707 M KOH needed to reach the equivalence point in the titration of 23.4 mL of 0.0390 M HNO2. Volume: mL KOH pH =
Be sure to answer all parts find the value of S . Report the value with...
Be sure to answer all parts find the value of S . Report the value with the appropriate sign. (a) 3 NO2( g ) + H2O( l ) 2 HNO3( l ) + NO( g ) J/K (b) N2( g ) + 3 F2( g ) 2 NF3( g ) J/K (c) C6H12O6( s ) + 6 O2( g ) 6 CO2( g ) + 6 H2O( g ) J/K
Be sure to answer all parts. At 430 ° C, the equilibrium constant (KP) for the...
Be sure to answer all parts. At 430 ° C, the equilibrium constant (KP) for the reaction 2NO(g) + O2(g) ⇆ 2NO2(g) is 1.5 × 105. In one experiment, the initial pressures of NO, O2, and NO2 are  7.4 × 10−3 atm, 4.2 × 10−2 atm, and 0.20 atm, respectively. Calculate QP and predict the direction that the net reaction will shift to reach equilibrium. What is QP for the experiment? In which direction will the system proceed to reach equilibrium?...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT