Answer: I think its White Dwarf? Due to it being final stage of a star before death it would fuse a lot of its mass into iron, but i'm no expert so tell me if i'm wrong
25m/100 seconds = 0.25m/sec
Answer:
0.1296 grams of aluminum reacted
Explanation:
Equation of reaction:
2Al + 6HCl = 2AlCl3 + 3H2
From the ideal gas equation
PV = nRT
n = PV/RT
P = (25.2/760)atm + 0.89atm = 0.923 atm
V = 190.6 ml = 190.6cm^3
R = 82.057cm^3.atm/gmol.K
T = 26°C = 26+273K = 299K
n = 0.923×190.6/82.057×299 = 0.0072 moles of H2
From the equation of reaction
3 moles of hydrogen gas is formed from 2 moles of aluminum
Therefore, 0.0072 moles of hydrogen gas is formed from (0.0072×2/3 = 0.0048) moles of aluminum
Number of moles of aluminum that reacted = 0.0048 moles
Mass of aluminum that reacted = number of moles × MW = 0.0048 × 27 = 0.1296 grams
Answer:
19.9 mol
Explanation:
Use <em>Avogadro’s number</em> to convert formula units of CaI₂ to moles of CaI₂.
1 mol CaI₂ ≡ 6.022 × 10²³ formula units CaI₂
Moles of CaI₂ = 1.20 × 10²⁵ × (1 /6.022 × 10²³)
Moles of CaI₂ = 19.9 mol
Answer:
The correct answer is -2878 kJ/mol.
Explanation:
The reaction that takes place at the time of the oxidation of glucose is,
C₆H₁₂O₆ (s) + 6O₂ (g) ⇒ 6CO₂ (g) + 6H₂O (l)
The standard free energy change for the oxidation of glucose can be determined by using the formula,
ΔG°rxn = ∑nΔG°f (products) - ∑nΔG°f (reactants)
The ΔG°f for glucose is -910.56 kJ/mol, for oxygen is 0 kJ/mol, for H2O -237.14 kJ/mol and for CO2 is -394.39 kJ/mol.
Therefore, ΔG°rxn = 6 (-237.14) + 6 (-394.39) - (-910.56)
ΔG°rxn = -2878 kJ/mol
