Answer:
It looks alittle dark can you fix it?
THe balanced chemical reaction would be:
Na2CO3 + H2SO4 = Na2SO4 + H2O + CO2
We first convert the mass of sulfuric acid solution to moles by the molar mass. Then, we relate H2SO4 with Na2CO3 from the reaction. We do as follows:
<span>6.05×10^3 kg H2SO4 ( 1 kmol / 98.08 kg) ( 1 kmol Na2CO3 / 1 kmol H2SO4 ) ( 105.99 kg / kmol ) = 6537.92 kg Na2CO3 needed</span>
We have to fill the gap
The correct answer is: Metals with the largest atoms and the smallest number of valence electrons and non-metals with the smallest atoms and the greatest number of valence electrons are the most reactive.
Reactivity of any species depends on ease of release or gain of electron. The species which can release electron easily from valence shell, the species is more reactive whereas the species which can accept electron to its valence shell easily is also more reactive.
Answer:
Detail is given below.
Explanation:
Chemical equation:
4NH₃ + 3O₂ → 2N₂ + 6H₂O
This reaction shows that when ammonia react with oxygen it form water and nitrogen gas.
There are two reactants on left hand side oxygen and ammonia. Ammonia is formed when nitrogen and hydrogen react. While on right hand side there are two products nitrogen and water. Water is formed by the reaction of hydrogen and oxygen.
The given reaction also shows that it follow the law of conservation of mass.
According to the law of conservation mass, mass can neither be created nor destroyed in a chemical equation.
This law was given by French chemist Antoine Lavoisier in 1789. According to this law mass of reactant and mass of product must be equal, because masses are not created or destroyed in a chemical reaction.
Answer:
8.1 × 10² g
Explanation:
Step 1: Write the balanced equation
2 C₅₇H₁₁₀O₆ + 163 O₂ ⇒ 114 CO₂ + 110 H₂O
Step 2: Convert 1.6 lb of C₅₇H₁₁₀O₆ to g
We will use the conversion factor 1 lb = 453.592 g.
1.6 lb × 453.592 g/1 lb = 7.3 × 10² g
Step 3: Calculate the moles corresponding to 7.3 × 10² g of C₅₇H₁₁₀O₆
The molar mass of C₅₇H₁₁₀O₆ is 890.83 g/mol.
7.3 × 10² g × 1 mol/890.83 g = 0.82 mol
Step 4: Calculate the moles of water produced from 0.82 moles of C₅₇H₁₁₀O₆
The molar ratio of C₅₇H₁₁₀O₆ to H₂O is 2:110. The moles of H₂O produced are 110/2 × 0.82 mol = 45 mol
Step 5: Calculate the mass corresponding to 45 moles of H₂O
The molar mass of H₂O is 18.02 g/mol.
45 mol × 18.02 g/mol = 8.1 × 10² g
