43 inHg = 43 inHg*2.54cm/in = 109.22cmHg * 10 mm/cm = 1092.2 mmHg
14.7 psi = 760 mmHg
1092.2mmHg * 14.7psi / 760 mmHg = 21.13 psi
Answer: option D. 21.13 psi
Answer:
248.4 mL
Explanation:
Erlenmeyer = 78.649 g
Erlenmeyer + Water = 327.039 g
Water = (Erlenmeyer + Water) - Erlenmeyer
Water = 327.039 - 78.649
Water = 248.4 g
if the density of water is 1 g/mL, we can say that each mL of water weigh 1 g, so we have 248.4 mL of water in the Erlenmeyer Flask.
Answer:
202 L
Explanation:
Step 1: Write the balanced equation
C₆H₁₂O₆ + 6 O₂(g) ⇒ 6 CO₂(g) + 6 H₂O(l)
Step 2: Calculate the moles corresponding to 270 g of C₆H₁₂O₆
The molar mass of C₆H₁₂O₆ is 180.16 g/mol.
270 g × 1 mol/180.16 g = 1.50 mol
Step 3: Calculate the moles of CO₂ generated from 1.50 moles of glucose
The molar ratio of C₆H₁₂O₆ to CO₂ is 1:6. The moles of CO₂ formed are 6/1 × 1.50 mol = 9.00 mol
Step 4: Calculate the volume of 9.00 moles of CO₂ at STP
The volume of 1 mole of an ideal gas at STP is 22.4 L.
9.00 mol × 22.4 L/mol = 202 L
Answer:
The answer to your question is below
Explanation:
Factors that affect the rate of a chemical reaction
- Temperature If the temperature increases the rate of reaction increases.
- Concentration The reaction will move where there less concentration it could be to the reactants of products.
- Particle size The lower the particle size the higher the rate of reaction.
- Catalyst Catalyzers accelerate the rate of reaction
- Pressure The reaction will move where there are fewer molecules.
Helium only possesses two valence electrons, while the other noble gasses posses eight