Answer:
8.934 g
Step-by-step explanation:
We know we will need a balanced equation with masses and molar masses, so let’s gather all the information in one place.
M_r: 192.12 44.01
H₃C₆H₅O₇ + 3NaHCO₃ ⟶ Na₃C₆H₅O₇ + 3H₂O + 3CO₂
m/g: 13.00
For ease of writing, let's write H₃C₆H₅O₇ as H₃Cit.
(a) Calculate the <em>moles of H₃Cit
</em>
n = 13.00 g × (1 mol H₃Cit /192.12 g H₃Cit)
n = 0.067 67 mol H₃Cit
(b) Calculate the <em>moles of CO₂
</em>
The molar ratio is (3 mol CO₂/1 mol H₃Cit)
n = 0.067 67 mol H₃Cit × (3 mol CO₂/1 mol H₃Cit)
n = 0.2030 mol CO₂
(c) Calculate the <em>mass of CO₂
</em>
m = 0.2030 mol CO₂ × (44.01 g CO₂/1 mol CO₂)
m = 8.934 g CO₂
Answer:
C) 11 g
Explanation:
first look to graph , you have x and y
x is mass of Fe
and y is mass of product
if the reaction consumes 2 g of Fe , ( look to x axis , look to 2 )
and go up until the black line touch the line of number 2
and go left and you will see the point become in the middle between 10 and 12
** 12 (11) 10 ***
Good Luck
Answer:
Ek = (RT/zF)*ln ( [k+]o/[K+]i )
Explanation:
R = gas constant (8.31 J/Kmol)
T = Temperature (k)
F = Faraday constant (9.65 * 10exp4 coulomb/mole)
z = valence of the ion (1)
[k+]o = Extracellular K concentration in mM
[K+]i = Intracellular K concentration in mM
ln = logarithm with base e
Hey There!
let see the definition of law of multiple proportions when two eliments combine to form more than one compound the mass of one element which combine with mass of other element is will always be a fixed ratio ,accordingly answer is first option.
Answer A : N2O , NO , NO2