Question

analysis: there will be 2 sections to your analysis listed below (calculations) fill out the data table above. all calculations needed to fill out the data table will need to be shown. every calculation. (calculations) use the bolded data and the pv=nrt equation to solve for the molar mass of the gas (g/mol). all calculations that are needed to determine the molar mass of the gas. every calculation conclusion: calculate a percent error for your experiment (butane = 58.12 g/mol). explain some experimental errors that could have occurred leading to a high error. do some research on the contents of butane lighters and explain why the molar mass calculation could have been inaccurate. (at least one paragraph)

Explanation:

Step1: Recall the ideal - gas law

The ideal - gas law is $PV = nRT$, where $P$ is pressure, $V$ is volume, $n$ is the number of moles, $R$ is the ideal - gas constant ($R=0.0821\ L\cdot atm/(mol\cdot K)$), and $T$ is temperature in Kelvin. We can express $n=\frac{m}{M}$, where $m$ is the mass of the gas and $M$ is the molar mass. So, $PV=\frac{m}{M}RT$, and we can solve for $M$: $M = \frac{mRT}{PV}$.

Step2: Identify given values

We need to identify the values of $P$, $V$, $m$, $T$ from the bolded data. Convert the units as necessary. For example, if pressure is in mmHg, convert it to atm ($1\ atm = 760\ mmHg$), if volume is in mL, convert it to L ($1\ L=1000\ mL$), and if temperature is in $^{\circ}C$, convert it to Kelvin ($T(K)=T(^{\circ}C)+ 273.15$).

Step3: Calculate molar mass

Substitute the values of $m$, $R$, $T$, $P$, and $V$ into the formula $M=\frac{mRT}{PV}$ and calculate the molar mass of the gas.

Step4: Calculate percent error

The percent - error formula is $\text{Percent Error}=\frac{\vert\text{Experimental Value}-\text{Theoretical Value}\vert}{\text{Theoretical Value}}\times100\%$. The theoretical value of the molar mass of butane is $58.12\ g/mol$. Substitute the experimental molar mass (calculated in Step 3) and the theoretical molar mass into the formula to find the percent error.

Step5: Analyze experimental errors

Possible experimental errors include:

• Leakage of gas: If there is a leak in the apparatus, the amount of gas measured will be less than the actual amount, leading to an incorrect molar - mass calculation.
• Inaccurate measurement of volume: Errors in reading the volume of the gas (e.g., parallax error when reading a graduated cylinder) can cause inaccuracies.
• Incorrect temperature or pressure measurements: Any error in measuring the temperature or pressure of the gas will affect the calculation of the number of moles using the ideal - gas law, and thus the molar mass.

Answer:

The molar mass of the gas can be calculated using $M = \frac{mRT}{PV}$. The percent error can be calculated using $\text{Percent Error}=\frac{\vert\text{Experimental Value}-\text{Theoretical Value}\vert}{\text{Theoretical Value}}\times100\%$. Experimental errors may include gas leakage, inaccurate volume, temperature, or pressure measurements.