Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced.Suppose the CO2 gas evolved by a certain chemical reaction taking place at 35.0°C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 34.9mL.Sketch of a gas-collection apparatusCalculate the mass of CO2 that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases.

To calculate the mass of CO2 in the collection tube, 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.

First, we need to convert the temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = °C + 273.15. So, 35.0°C = 35.0 + 273.15 = 308.15 K.

Next, we need to convert the volume from mL to L because the ideal gas constant R is usually given in L·atm/(mol·K). The conversion is 1 L = 1000 mL, so 34.9 mL = 34.9/1000 = 0.0349 L.

The pressure of the gas is the sum of the partial pressure of CO2 and the vapor pressure of water at 35.0°C. We can assume that the partial pressure of CO2 is approximately equal to the atmospheric pressure because CO2 is much denser than water vapor. The atmospheric pressure at sea level is about 1 atm. The vapor pressure of water at 35.0°C is about 0.0422 atm. So, the total pressure P = 1 - 0.0422 = 0.9578 atm.

Now we can calculate the number of moles of CO2 using the ideal gas law equation. Rearranging the equation to solve for n, we get n = PV/RT. Substituting the known values, we get n = (0.9578 atm)(0.0349 L) / ((0.0821 L·atm/(mol·K))(308.15 K)) = 0.00137 mol.

Finally, we can calculate the mass of CO2 by multiplying the number of moles by the molar mass of CO2. The molar mass of CO2 is about 44.01 g/mol. So, the mass of CO2 = (0.00137 mol)(44.01 g/mol) = 0.060 g.

So, the mass of CO2 in the collection tube is approximately 0.060 g, rounded to two significant digits.

To calculate the mass of CO2 in the collection tube, 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.

Step 1: Convert the temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = °C + 273.15. So, 35.0°C = 308.15 K.

Step 2: Convert the volume from mL to L. The conversion factor is 1 L = 1000 mL. So, 34.9 mL = 0.0349 L.

Step 3: Assume the pressure to be 1 atm, which is a normal and reasonable assumption for lab conditions.

Step 4: Use the ideal gas constant R = 0.0821 L·atm/K·mol.

Step 5: Substitute the values into the ideal gas law equation and solve for n (number of moles):

1 atm * 0.0349 L = n * 0.0821 L·atm/K·mol * 308.15 K

Solving for n gives n = 0.0014 moles.

Step 6: Convert moles of CO2 to grams. The molar mass of CO2 is approximately 44.01 g/mol. So, 0.0014 moles * 44.01 g/mol = 0.062 g.

Therefore, the mass of CO2 in the collection tube is approximately 0.062 g.

To calculate the mass of CO2 in the collection tube, we need to use the ideal gas law equation, PV = nRT, where:

P = pressure V = volume n = number of moles R = ideal gas constant T = temperature

First, we need to convert the temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = °C + 273.15. So, 35.0°C = 308.15 K.

Next, we need to know the pressure. Since the problem doesn't provide this, we'll assume standard atmospheric pressure, which is 1 atm.

The volume of the gas is given as 34.9 mL, which we need to convert to liters (since the ideal gas constant R uses liters). So, 34.9 mL = 0.0349 L.

The ideal gas constant R is 0.0821 L·atm/(K·mol).

Now we can solve for n (number of moles) using the ideal gas law:

n = PV/RT n = (1 atm)(0.0349 L) / (0.0821 L·atm/(K·mol) * 308.15 K) n = 0.0014 moles

Finally, to find the mass of the CO2, we multiply the number of moles by the molar mass of CO2 (which is about 44.01 g/mol):

mass = n * molar mass mass = 0.0014 moles * 44.01 g/mol mass = 0.062 g

So, the mass of CO2 in the collection tube is approximately 0.062 g.