Answer:
22.1 g
Explanation:
Step 1: Write the balanced equation for the combustion of acetylene
2 C₂H₂ + 5 O₂ ⇒ 4 CO₂ + 2 H₂O
Step 2: Calculate the moles corresponding to 75.0 g of CO₂
The molar mass of CO₂ is 44.01 g/mol.
75.0 g × 1 mol/44.01 g = 1.70 mol
Step 3: Calculate the moles of C₂H₂ required to produce 1.70 moles of CO₂
The molar ratio of C₂H₂ to CO₂ is 2:4. The moles of C₂H₂ required are 2/4 × 1.70 mol = 0.850 mol.
Step 4: Calculate the mass corresponding to 0.850 moles of C₂H₂
The molar mass of C₂H₂ is 26.04 g/mol.
0.850 mol × 26.04 g/mol = 22.1 g
D- the uneven heating causes global wind patterns
Answer : If any atom has more electrons than one energy level can hold, then automatically the electron is accommodated in the next energy level (shell). The remaining extra electrons starts to fill the next energy level. This produces the valency of that particular atom.
If data results a reproducible but not accurate, it means that there was a high level of precision, but not complete accuracy.
<u>Answer:</u> The value of equilibrium constant for the given reaction at 517 K is 1.30
<u>Explanation:</u>
The chemical equation for the dissociation of follows:
The expression of for above equation follows:
We are given:
Putting values in above expression, we get:
Hence, the value of equilibrium constant for the given reaction at 517 K is 1.30