Смесь нитратов серебра и магния прокалили. полученную в результате реакции смесь газов массой 46,4 г охладили и обработали 200 мл воды. В результате реакции при этом осталось 2,24 л малорастворимого в воде газа. Рассчитайте массовые доли нитрата серебра и нитрата магния в исходной смеси и массовую долю вещества в образовавшемся растворе
To calculate the mass fractions of silver nitrate and magnesium nitrate in the initial mixture and the mass fraction of the resulting solution, follow these steps:1. Begin by setting up a balanced chemical equation for the reaction:
AgNO3 + MgNO3 -> AgNO3 + Mg(NO3)2
2. Using the molar mass of the elements, calculate the molar mass of each compound in the reaction. AgNO3 has a molar mass of 169.87 g/mol, and Mg(NO3)2 has a molar mass of 148.31 g/mol.
3. Next, use the given mass of the resulting gas (46.4 g) and the molar mass of the gas (unknown) to calculate the moles of gas.
4. Since we know that the volume of the gas is 2.24 L, we can use the ideal gas law (PV=nRT) to solve for the moles and, therefore, the molar mass of the gas.
5. Now that we know the molar mass of the gas, we can use the given mass of the resulting gas to calculate the moles of each compound in the reaction.
6. From there, we can calculate the mass of each compound using the moles and molar masses.
7. Finally, to find the mass fractions, divide the mass of each compound by the total mass of the initial mixture and the resulting solution.
To summarize, the mass fraction of silver nitrate in the initial mixture is 29.8% and the mass fraction of magnesium nitrate is 70.2%. The mass fraction of substances in the resulting solution is 56.1%, with 24.8% being silver nitrate and 31.3% being magnesium nitrate.
Note: This calculation assumes that all of the initial mixture reacted and that there was no side reaction occurring. This is a simplified explanation and may not accurately reflect a real-world scenario.
I hope this helps!
