Answer:
The forward reaction is spontaneous above 533 K.
Explanation:
A reaction is spontaneous when the standard Gibbs energy of the reaction (ΔG°) is negative. ΔG° is related to the standard enthalpy of the reaction (ΔH°) and the standard entropy of the reaction (ΔS°) through the following expression.
ΔG° = ΔH° - T.ΔS°
where,
T is the absolute temperature
When ΔG° < 0,
ΔH° - T.ΔS° < 0
ΔH° < T.ΔS°
T > ΔH° / ΔS° = (67.7 × 10³ J) / (126.9 J/K) = 533 K
The forward reaction is spontaneous above 533 K.
0.1324 ×10^24 atoms of carbon are in 2.65 g of carbon
Explanation:
Converting the grams of carbon to the moles of carbon.
Divide the mass (2.65 g) by 12.011 g/mol which is the molecular weight of carbon,
2.65 g / 12.011 g/mol=0.220 moles of carbon
Then, convert moles of carbon to atoms of carbon using Avogadro's constant (6.022×10^23 atoms per mole)
0.220 moles × 6.022×10^23 atoms / 1 mole = 0.1324 ×10^24 atoms
0.1324 ×10^24 atoms of carbon are in 2.65 g of carbon
Answer: the concentration of H in the stomach acid is greater than that of the lemon juice
Explanation:Please see attachment for explanation
A) 36.0 x 100 /2 = 1800 g Be
n = m / MM
stoichiometry 1:1
atomic mass of Be= 100 g/ mol
b) theoretical yield