sorry for the bad photo, but #6 is the one I need help with **Educational Content:**---**Section 5:**- A 256-mL flask containing air has a mass of 119.2861 g. If the mass of the flask filled with water is 378.26 g, what is the volume of air in the flask? (Density of water = 0.9975 g/mL) **Solution Steps:** \[ \text{Mass of water} = 378.26 \text{ g} - 119.2861 \text{ g} = 258.9739 \text{ g} \] Using the density of water: \[ \text{Volume of water} = \frac{258.9739 \text{ g}}{0.9975 \text{ g/mL}} = 259.6 \text{ mL} \]**Section 6:**- What is the volume of a gas at standard conditions (STP) if the volume at 1.014 atm and 286.7 K is 246.7 mL? **Conditions:** \[ \text{Initial Pressure} = 1.014 \text{ atm} \] \[ \text{Initial Temperature} = 286.7 \text{ K} \] \[ \text{Initial Volume} = 246.7 \text{ mL} \] Using the ideal gas law or relevant formulas, calculate the volume at STP, integrating changes in pressure and temperature.**Section 7:**- Assuming natural gas is entirely methane (CH₄), what would the density be at standard conditions? \[ \text{Molar mass of methane} = 16.04 \text{ g/mol} \] Further calculations would involve using the ideal gas law for density determination at standard conditions.--- **Note:** Ensure all calculations are cross-verified for accuracy and comprehensiveness in educational scenarios. Use this template for educational purposes and not as a final definitive calculation without proper validation from scientific practices.

At standard temperature and pressure, a system is said to have a temperature of 0°C or 273.15 K and the pressure equal to the atmosphere is always 1 atm. Additionally, one mole of any gas at STP occupies a volume of 22.414 L. This concept only holds true for gases.Here, we will calculate the volume of a gas at standard conditions. We will use the formula to find the volume of a gas is- P1V1T1=P2V2T2..................(1) It is given that, P1=1.014 atmT1=286.7 KV=246.7 ml In STP condition, P2=1 atmT2=273.15 KV2=? Put all values in above formula (1). 1.014 atm×246.7 ml286.7 K=1 atm×V2273.15 KV2=1.014×246.7×273.151×286.7=238.33 ml Therefore, the volume of a gas at standard condition is 238.33 ml.