What is the average of atomic mass of carbon if 98.90% of the atoms are c-12 and 1.100% are c-13 atoms?
1 answer:
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Answer:
a) The slope of the line of best fit plot = -12629.507
b) ΔH∘ = 105 kJ
c) Intercept of the line of best fit plot = 39.099
d) ΔS∘ = 325.1 J/K
e) Option A is correct.
Solubility will increase as temperature increases, because as T increases the (−ΔH∘/RT) term becomes smaller therefore K will get larger.
f) Option D is correct. All of the options are correct.
Explanation:
The complete question is presented in the first attached image to this question. This complete question has the data readings required to plot the graph.
The second attached image has the plotted graph and the regression analysis to obtain the line of best fit.
The equation of the line of best fit obtained is
y = -12629.507x + 39.099
Comparing the given expression for the question with the equation of a straight line
ln (K) = (−ΔH∘/RT) + (ΔS∘/R)
y = mx + c
y = In K
Slope = m = (−ΔH∘/R)
x = (1/T)
Intercept = c = (ΔS∘/R)
So, to answer the question now
a) The slope of the line of best fit plot = -12629.507
b) Slope = (−ΔH∘/R)
(−ΔH∘/R) = -12629.507
But R = molar gas constant = 8.314 J/mol.K
ΔH∘ = 12629.507 × 8.314 = 105,001.721198 J = 105,002 J = 105 kJ
c) Intercept of the line of best fit plot = 39.099
d) Intercept = (ΔS∘/R)
(ΔS∘/R) = 39.099
ΔS∘ = 39.099 × 8.314 = 325.069086 J/K = 325.1 J/K
e) Do you expect the solubility of Borax to increase or decrease as temperature increases?
Solubility will increase as temperature increases, because as T increases the (−ΔH∘/RT) term becomes smaller therefore K will get larger.
f) Why was it necessary to make sure that some solid was present in the main solution before taking the samples to measure Ksp? Select the option that best explains why.
A. To make sure no more sodium borate would dissolve in solution.
B. To ensure the dissolution process was at equilibrium.
C. To make sure the solution was saturated with sodium and borate ions.
D. All of the above
Hope this Helps!!!
Answer:
Oxide of M is and sulfate of
Explanation:
0.303 L of molecular hydrogen gas measured at 17°C and 741 mmHg.
Let moles of hydrogen gas be n.
Temperature of the gas ,T= 17°C =290 K
Pressure of the gas ,P= 741 mmHg= 0.9633 atm
Volume occupied by gas , V = 0.303 L
Using an ideal gas equation:
Moles of hydrogen gas produced = 0.01225 mol
Moles of metal =
So, 8.3333 mol of metal M gives 0.01225 mol of hydrogen gas.
x = 2.9 ≈ 3
Formulas for the oxide and sulfate of M will be:
Oxide of M is and sulfate of
.