2.5 x 10-2 L
25 m3
The heat of the reaction can be calculated using the enthalpy of formation. For a 53.99-g sample of iron, the heat of the reaction is approximately -798.9 kJ.
To calculate the heat of the reaction, we need to use the concept of enthalpy of formation. The enthalpy of formation of Fe2O3(s) is -826.0 kJ/mol. We can use this value as a conversion factor to find the heat produced when 1 mole of Fe2O3(s) is formed. Since we have a 53.99-g sample of iron, we can calculate the moles of iron and use the conversion factor to find the heat of the reaction.
The molar mass of iron (Fe) is 55.845 g/mol. Therefore, the moles of iron in the sample can be calculated as:
(53.99 g) / (55.845 g/mol) = 0.9662 mol
Now, using the conversion factor:
0.9662 mol Fe × (826.0 kJ/mol) = -798.9 kJ
Therefore, the heat of the reaction 4Fe(s) + 3O2(g) → 2Fe2O3(s) when a 53.99-g sample of iron is reacted is approximately -798.9 kJ.
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The problem is solved by first converting the given mass of Fe to moles, then determining the amount of Fe2O3 formed using the stoichiometry of the reaction. With the heat formation of Fe2O3 given, the heat released in the reaction is calculated to be -399.8 kJ, indicating an exothermic reaction.
To solve the given problem, we first need to calculate the number of moles of Fe in the 53.99-g sample. The molar mass of Fe is about 55.85 g/mol, so 53.99 grams will represent approximately 0.967 moles of iron. Given the reaction 4Fe + 3O2 → 2Fe2O3, the formation of 2 moles of Fe2O3 requires 4 moles of Fe; hence a ratio of 2:4= 0.5:1 is formed. So, from 0.967 moles of iron, we get 0.967*0.5 = 0.484 moles of Fe2O3 formed.
From the problem, we know that the heat of formation of Fe2O3 is -826.0 kJ/mol. Therefore, the heat of reaction or released heat from the formation of 0.484 moles will be 0.484*-826.0 kJ/mol = -399.8 kJ. Because the value is negative, this is an exothermic reaction, releasing heat.
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When the temperature of a substance decreases, the average kinetic energy of its particles also decreases. This is because the temperature of a substance is proportional to the average kinetic energy of its particles. The slower the particles move, the lower the kinetic energy.
The question refers to the relationship between the temperature of a substance and the average kinetic energy of its particles. According to the kinetic-molecular theory, the temperature of a substance is proportional to the average kinetic energy of its particles. When the temperature of a substance rises, the particles vibrate more in solids or move more rapidly in liquids and gases, indicating an increase in kinetic energy. Conversely, if the temperature decreases, the kinetic energy also decreases, and the particles move more slowly.
For instance, when the temperature of a gas increases, its average kinetic energy increases, more molecules have higher speeds and fewer molecules have lower speeds. The distribution shifts towards higher speeds overall. If the temperature decreases, the opposite happens: the average kinetic energy decreases, more molecules have lower speeds and fewer molecules have higher speeds. The distribution shifts towards lower speeds overall.
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Answer:
3.56L will be the obtained volume
Explanation:
0.3 M → Molarity
These are the moles of solute (for this case, the solute is KOH) that are contianed in 1L of solution
We dissolved 60 g of solute, so let's determine the moles:
60 g . 1 mol/ 56.1 g = 1.07 moles
Molarity(mol/L) = Mol / Volume(L)
Let's replace data: 0.3M = 1.07 mol / Volume(L)
0.3 mol/L = 1.07 mol / volume
Volume = 1.07 mol / 0.3mol/L = 3.56 L
(2) 7 (4) 4
The given formula MgSO₄•7H₂O contains 11 oxygen atoms. Therefore, option (1) is correct.
A chemical formula of a compound describes the chemical proportions of each element in a chemical compound or molecule. The chemical formula of a molecule can be written with help of the chemical symbols of elements, numbers (subscripts), and some other symbols, such as brackets, dashes, plus (+) and minus (−) signs, and commas.
A chemical formula contains no words but contains certain simple chemical structures but not complete structures. These formulae must be limited in power than chemical names and structural formulae.
We have two types of formulas in chemistry one empirical formula and the other molecular formula. In the formula MgSO₄•7H₂O, the four oxygen atoms in MgSO₄ and seven from 7 water molcules.
The number of oxygen atoms in the given formula MgSO₄•7H₂O is equal to (4 + 7) = 11 atoms.
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I got you my friend.
mass = 42.3 kg
If you want step by step let me know in the comments and ill post a step by step in the comment section.