Final answer:
The question requires calculating the mass of water that can be heated using the heat from the combustion of ethane. Utilizing the provided enthalpy change and the specific heat capacity of water, the correct calculation provides a mass of water not listed in the options. It suggests an error in the options or a potential missing piece of information.
Step-by-step explanation:
The question asks how many kilograms of water can be heated from 10°C to 50°C using the heat from the combustion of ethane (C2H6). To solve this, we can use the formula: \(q = m \cdot c \cdot \Delta{T}\), where \(q\) is the heat transferred, \(m\) is the mass of the water, \(c\) is the specific heat capacity of water (4.18 kJ/kg°C), and \(\Delta{T}\) is the change in temperature. Given that \(\Delta{H}\) for the combustion of ethane is -1559.8 kJ/mol and the temperature change required is 40°C (from 10°C to 50°C), we can set up the following equation:
\(-1559.8 kJ = m \cdot 4.18 kJ/kg°C \cdot 40°C\)
Solving for \(m\), we find that \(m\) is approximately \(9.33 kg\), which is not an option in the given choices. As this is a high school chemistry problem, it is essential to ensure that all necessary information is provided and that calculations are carried out correctly.