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qwelly [4]
3 years ago
8

A baker uses sodium hydrogen carbonate (baking soda) as the leavening agent in a banana-nut quick bread. the baking soda decompo

ses according to two possible reactions. reaction 1: 2 nahco3(s) → na2co3(s) + h2o(l) + co2(g) reaction 2: nahco3(s) + h+(aq) → h2o(l) + co2(g) + na+(aq) calculate the volume (in ml) of co2 that forms at 170.°c and 0.900 atm per gram of nahco3 by each of the reaction processes.
Chemistry
1 answer:
Kamila [148]3 years ago
6 0

Answer : The volume of CO_2 in Reaction 1 = 240.45 ml

The volume of CO_2 in Reaction 2 = 480.89 ml

Solution : Given,

Temperature = 170^oC=170+273=443K         (1^oC=273K)

Pressure = 0.900 atm

The mass of NaHCO_3 = 1 gram

Molar mass of NaHCO_3 = 84.007 g/mole

The given reactions are,

Reaction 1 : 2NaHCO_3(s)\rightarrow Na_2CO_3(s)+H_2O(l)+CO_2(g)

Reaction 2 : NaHCO_3(s)+H^+(aq)\rightarrow H_2O(l)+CO_2(g)+Na^+(aq)

  • <u>Calculation for Reaction 1 :</u>

First we have to calculate the moles of NaHCO_3.

Moles of NaHCO_3 = \frac{1g}{84.007g/mole}=0.0119moles

From the Reaction 1, we conclude that

2 moles of NaHCO_3 gives 1 mole of CO_2

0.0119 moles of NaHCO_3 gives \frac{1mole}{2moles}\times 0.0119moles=0.00595moles of CO_2

Using ideal gas equation :  

PV=nRT\\V=\frac{nRT}{P}

where,

P = pressure of gas

V = volume of gas

n = Number of moles

T = temperature of gas

R = gas constant = 0.0821 L atm/mole K

Now put all the given values in ideal gas law, we get the volume of CO_2

V=\frac{(0.00595mole)\times (0.0821Latm/moleK)\times 443K}{0.900atm}=0.24045L=240.45ml

The volume of CO_2 in Reaction 1 is 240.45 ml

  • <u>Calculation for Reaction 2 :</u>

The moles of NaHCO_3 = 0.0119 moles

From the Reaction 2, we conclude that

1 moles of NaHCO_3 gives 1 mole of CO_2

So, the moles of CO_2 = the moles of NaHCO_3 = 0.0119 moles

Using ideal gas equation,

PV=nRT\\V=\frac{nRT}{P}

Now put all the given values in ideal gas law, we get the volume of CO_2

V=\frac{(0.0119mole)\times (0.0821Latm/moleK)\times 443K}{0.900atm}=0.48089L=480.89ml

The volume of CO_2 in Reaction 2 is 480.89 ml


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Balance the following redox reaction occurring in an acidic solution. The coefficient of Mn2+(aq) is given. Enter the coefficien
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Answer:

_5_ AsO2−(aq) + 3 Mn2+(aq) + _2_ H2O(l) → _5_ As(s) + _3_ MnO4−(aq) + _4_ H+(aq)

Explanation:

Step 1:

The unbalanced equation:

AsO2−(aq) + 3 Mn2+(aq) + H2O(l) → As(s) + MnO4−(aq) + H+(aq)

Step 2:

Balancing the equation.

AsO2−(aq) + 3Mn2+(aq) + H2O(l) → As(s) + MnO4−(aq) + H+(aq)

The above equation can be balanced as follow:

There are 3 atoms of Mn on the left side of the equation and 1 atom on the right side. It can be balance by putting 3 in front of MnO4− as shown below:

AsO2−(aq) + 3Mn2+(aq) + H2O(l) → As(s) + 3MnO4−(aq) + H+(aq)

There are 12 atoms of O on the right side and a total of 3 atoms on the left side. It can be balance by putting 5 in front of AsO2− and 2 in front of H2O as shown below:

5AsO2−(aq) + 3Mn2+(aq) + 2H2O(l) → As(s) + 3MnO4−(aq) + H+(aq)

There are 4 atoms of H on the left side and 1 atom on the right side. It can be balance by putting 4 in front of H+ as shown below:

5AsO2−(aq) + 3Mn2+(aq) + 2H2O(l) → As(s) + 3MnO4−(aq) + 4H+(aq)

There are 5 atoms of As on the left side and 1 atom on the right side. It can be balance by putting 5 in front of As as shown below:

5AsO2−(aq) + 3Mn2+(aq) + 2H2O(l) → 5As(s) + 3MnO4−(aq) + 4H+(aq)

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3 years ago
A sample of oxygen gas has a volume of 3.24 L at 29°C. What volume will it occupy at 104°C if the pressure and number of mol are
ohaa [14]

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<u>Explanation:</u>

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Mathematically,

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Putting values in above equation, we get:

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