The reaction of calcium bicarbonate, Ca(HCO3)2 with hydrochloric acid, HCl, produces a solution of CaCl2, gaseous carbon dioxide, CO2, and water, H2O. Write a balanced chemical equation for this reaction and determine the volume of CO2, in mL, that forms at 30.0 oC and 0.660 atm upon reacting 40.3 mL of 0.200 M Ca(HCO3)2 with excess HCl.

I. balanced equation:

Ca(HCO3)2 + HCl ->CaCl2 + 2 H2O + 2 CO2

II. find moles of Ca(HCO3)2 :

40.3 mL x 1 L/1000mL x 0.2 mole/L =
8.06 x 10^-3 moles Ca(HCO3)2

III. find moles CO2 :
[8.06 x 10^-3] moles Ca(HCO3)2 x
2 moles CO2/1 mole Ca(HCO3)2 =
1.61 x 10^-2 moles CO2

IV. find volume from PV=nRT
V= nRT/P
V = (1.61 x10^-2)(0.082)(273 +30)
all divided by 0.660) = 0.606 L =606 mL

To write a balanced chemical equation for the reaction between calcium bicarbonate and hydrochloric acid, we need to consider the formulas of the compounds involved and their charges.

The formula for calcium bicarbonate is Ca(HCO3)2, which contains the calcium ion (Ca^2+) and two bicarbonate ions (HCO3^-). The formula for hydrochloric acid is HCl, which contains the hydrogen ion (H^+) and the chloride ion (Cl^-).

The balanced chemical equation for the reaction can be written as follows:

Ca(HCO3)2 + 2 HCl -> CaCl2 + 2 CO2 + 2 H2O

Now, let's determine the volume of CO2 gas that forms at 30.0 °C and 0.660 atm when 40.3 mL of 0.200 M Ca(HCO3)2 reacts with excess HCl.

To solve this problem, we need to use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, we need to calculate the number of moles of Ca(HCO3)2 using its concentration and volume.

n(Ca(HCO3)2) = concentration × volume
n(Ca(HCO3)2) = 0.200 M × 0.0403 L
n(Ca(HCO3)2) = 0.00806 moles

Since the balanced chemical equation shows that 1 mole of Ca(HCO3)2 produces 2 moles of CO2, we can determine the number of moles of CO2 produced.

n(CO2) = 2 × n(Ca(HCO3)2)
n(CO2) = 2 × 0.00806 moles
n(CO2) = 0.01612 moles

Next, we convert the temperature from Celsius to Kelvin by adding 273.15.

T = 30.0 °C + 273.15
T = 303.15 K

Now, we can use the ideal gas law equation to calculate the volume of CO2 at the given conditions.

PV = nRT
V(CO2) = (n(CO2) × R × T) / P
V(CO2) = (0.01612 moles × 0.0821 L·atm/(mol·K) × 303.15 K) / 0.660 atm
V(CO2) ≈ 18.99 L

Finally, we convert the volume from liters to milliliters by multiplying by 1000.

V(CO2) = 18.99 L × 1000 mL/L
V(CO2) ≈ 18,990 mL

Therefore, approximately 18,990 mL of CO2 gas will form at 30.0 °C and 0.660 atm when 40.3 mL of 0.200 M Ca(HCO3)2 reacts with excess HCl.

The balanced chemical equation for the reaction between calcium bicarbonate and hydrochloric acid can be written as:

Ca(HCO3)2 + 2HCl -> CaCl2 + 2CO2 + 2H2O

To determine the volume of CO2 produced, we need to use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (in Kelvin)

First, we need to determine the number of moles of Ca(HCO3)2 used. To do this, we'll use the given volume and concentration information:

Volume of Ca(HCO3)2 = 40.3 mL = 0.0403 L
Concentration of Ca(HCO3)2 = 0.200 M

Number of moles of Ca(HCO3)2 = volume x concentration
n(Ca(HCO3)2) = 0.0403 L x 0.200 mol/L
n(Ca(HCO3)2) = 0.00806 mol

From the balanced chemical equation, we see that 2 moles of CO2 are produced for every 1 mole of Ca(HCO3)2. Thus, the number of moles of CO2 produced will also be 0.00806 mol.

Next, we need to convert the temperature from Celsius to Kelvin:

Temperature in Kelvin = 30.0 + 273.15
Temperature in Kelvin = 303.15 K

We are given the pressure of CO2 as 0.660 atm.

Using the ideal gas law equation, we can now calculate the volume of CO2:

PV = nRT

V(CO2) = n(CO2) x (R x T) / P
V(CO2) = 0.00806 mol x (0.0821 L.atm/mol.K x 303.15 K) / 0.660 atm
V(CO2) ≈ 0.098 L

Finally, we need to convert this volume from liters to milliliters:

Volume of CO2 in mL = V(CO2) x 1000 mL/L
Volume of CO2 in mL ≈ 98 mL

Therefore, the volume of CO2 formed is approximately 98 mL.