The total pressure of the gaseous mixture has been 5.37 atm. Thus, option D is correct.
The partial pressure has been defined as the pressure exerted by each gas in the mixture.
According to the Dalton's law of partial pressure, the total pressure of gas has been the sum of the partial pressure of the gases in the mixture.
The given partial pressure of gases in the mixture has been:
- Partial pressure of Nitrogen,

- Partial pressure of Oxygen,

- Partial pressure of Argon,

- Partial pressure of Helium,

- Partial pressure of Hydrogen,

The total pressure of the gaseous mixture has been:

The total pressure of the gaseous mixture has been 5.37 atm. Thus, option D is correct.
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Use the equation d = m/v or density equals mass over volume. 420/50.4=8.3333 or 8 and one third.
Answer:
The answer to your question is 1544 g of CO₂
Explanation:
Data
mass of octane = 500 g
mass of CO₂ = ?
Balanced chemical reaction
2C₈H₁₈ + 25O₂ ⇒ 16CO₂ + 18H₂O
Process
1.- Calculate the molar mass of octane and of carbon dioxide
C₈H₁₈ = 2[(12 x 8) + (1 x 18)] = 2[(96 + 18] = 2[114] = 228 g
CO₂ = 16[(12 x 1) + (16 x 2)] = 16[12 + 32] = 16[44] = 704 g
2.- Calculate the mass of carbon dioxide produced
228 g of C₈H₁₈ ---------------- 704 g of CO₂
500 g of C₈H₁₈ --------------- x CO₂
x = (500 x 704) / 228
x = 352000/228
x = 1544 g of CO₂
Answer:
the book absobes heat and the glass is reflection
Explanation: