Answer:
a-294
b-3.401×10^-6
c and d - 2.048×10^18
Explanation:
Multiply the RAM for each individual element by its molecular number, e.g., (c-12×14), and then sum to find the molar mass.
b-The molar mass is expressed in grams/mol, hence convert 1 mg to g, which equals 0.001, and divide it by the molar mass.
c/d-1 mole of any substance consists of 6.023×10^23 (ions, molecules, etc.), therefore we need to find the moles here as
(3.401×10^-6) × (6.023×10^23).
2C6H14 + 13O2 ---> 6CO2 +14H2O
Calculating the molar mass of C6H14: M(C6H14)=12.011*6 +1.008*14 ≈ 86.17 g/mol
Thus, 86.17 g of C6H14 corresponds to 1 mole.
2C6H14 + 13O2 ---> 6CO2 +14H2O
based on the equation 2 mol 6 mol
according to the question 1 mol 3 mol
To determine M(CO2): M(CO2)= 12.011 + 2*15.999= 44.009 g/mol
Therefore, 3 mol CO2*44.009 g/1 mol CO2 ≈ 132.0 g CO2
Final answer: 132.0 g CO2
Sr(s)+Mg²+(aq)→Sr²+(aq)+Mg(s)
Number of electrons transferred, n=2. Equilibrium constant,
K=2.69×10∧12
ΔG=-2.303RT logK
R=gas constant=8.314J/mol-k
T= temperature in K= 25°C=25+273=298K
Calculating gives us ΔG = -70922.3J. However, ΔG = -nFE
n= number of electrons transferred in the reaction =2
F= faraday = 96500C
E=cell potential is what?
∴E = ΔG.nF
=-(-70922.3)/2×96500)
=0.367V.
Answer: second option: 1.70 to 1.40
Explanation:
1) pH is defined using the formula pH = - log [H₃O⁺]
2) Given that the initial concentration is x and after doubling it becomes 2x, we calculate:
pHi = - logx
pHf = - log 2x = - log 2 - logx
Thus, pHf - pHi = - log2 - logx - (- logx) = - log2 ≈ - 0.30
⇒ pHi - pHf = 0.30, indicating that the final pH (with twice the hydronium ions) is 0.30 lower than the starting pH.
3) The only option that indicates a 0.30 decline in pH is the second one: from 1.70 to 1.40. Therefore, that is the correct choice.
