Answer:
This type of meat is substance. If you were talking about meters then it would be a system of measurement.
Answer:
Ionic bond
Explanation:
This type of chemical bond is called an ionic bond because the bond formed between two ions of opposite charge. The sodium cation (Na+) and the chlorine anion (Cl-) are attracted to one another to form sodium chloride, or table salt.
Answer:
41.54 grams of oxygen are required to burn 13.5 g of acetylene
Explanation:
The balanced reaction is:
2 C₂H₂ + 5 O₂ → 4 CO₂ + 2 H₂O
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- C₂H₂: 2 moles
- O₂: 5 moles
- CO₂: 4 moles
- H₂O: 2 moles
Being the molar mass of the compounds:
- C₂H₂: 26 g/mole
- O₂: 32 g/mole
- CO₂: 44 g/mole
- H₂O: 18 g/mole
By reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
- C₂H₂: 2 moles* 26 g/mole= 52 grams
- O₂: 5 moles* 32 g/mole= 160 grams
- CO₂: 4 moles* 44 g/mole= 176 grams
- H₂O: 2 moles* 18 g/mole= 36 grams
You can apply the following rule of three: if by stoichiometry 52 grams of acetylene react with 160 grams of oxygen, 13.5 grams of acetylene react with how much mass of oxygen?
![mass of oxygen=\frac{13.5 grams of acetylene*160 grams of oxygen}{52 grams of acetylene}](https://tex.z-dn.net/?f=mass%20of%20oxygen%3D%5Cfrac%7B13.5%20grams%20of%20acetylene%2A160%20grams%20of%20oxygen%7D%7B52%20grams%20of%20acetylene%7D)
mass of oxygen= 41.54 grams
<u><em>41.54 grams of oxygen are required to burn 13.5 g of acetylene</em></u>
<u><em></em></u>
Mass of Hydrogen gas produced : 3.202 g
<h3>Further explanation</h3>
A reaction coefficient is a number in the chemical formula of a substance involved in the reaction equation. The reaction coefficient is useful for equalizing reagents and products.
Hydrogen gas can be obtained by reacting metals with acids
Reaction of Aluminium(Al) and Hydrochloric acid(HCl)
2Al + 6HCl → 2AlCl₃ + 3H₂
mass of Aluminium : 28.56 g, so mol Al :
![\tt \dfrac{28.56}{26.98}=1.059~moles](https://tex.z-dn.net/?f=%5Ctt%20%5Cdfrac%7B28.56%7D%7B26.98%7D%3D1.059~moles)
From equation, mol ratio of Al : H₂ = 2 : 3, so mol H₂ :
![\tt \dfrac{3}{2}\times 1.059=1.5885](https://tex.z-dn.net/?f=%5Ctt%20%5Cdfrac%7B3%7D%7B2%7D%5Ctimes%201.059%3D1.5885)
Mass of Hydrogen gas produced :
![\tt mass=mol\times MW\\\\mass=1.5885\times 2.016\\\\mass=3.202~g](https://tex.z-dn.net/?f=%5Ctt%20mass%3Dmol%5Ctimes%20MW%5C%5C%5C%5Cmass%3D1.5885%5Ctimes%202.016%5C%5C%5C%5Cmass%3D3.202~g)
4NH3+5O2 <=>4NO + 6H2O
Using the definition of Kp, we have
Kp=(Pno^4*Ph2o^6)/(Pnh3^4*Po2^5)
where Pno=partial pressure of NO, etc.
The numerical value for a given temperature can be evaluated when the actual partial pressures are known.