Answer:
0.0907 M
Explanation:
Before you can calculate the molarity, you need to convert grams to moles (via molar mass) and convert mL to L.
(Step 1)
Molar Mass (C₈H₅O₄K):
8(12.011 g/mol) + 5(1.008 g/mol) + 4(15.998 g/mol) + 39.098 g/mol
Molar Mass (C₈H₅O₄K): 204.218 g/mol
0.6013 g C₈H₅O₄K 1 mole
------------------------------ x ------------------ = 0.00294 moles C₈H₅O₄K
204.218 g
(Step 2)
1,000 mL = 1 L
32.47 mL 1 L
--------------- x ----------------- = 0.03247 L
1,000 mL
(Step 3)
Molarity (M) = moles / volume (L)
Molarity = 0.00294 moles / 0.03247 L
Molarity = 0.0907 M
Answer:
299.14 K or 26°C
Explanation:
The ideal gas law, also called the general gas equation, is the equation of state of a hypothetical ideal gas.
The ideal gas law is often written as
PV = nRT
where P ,V and T are the pressure, volume and absolute temperature;
n is the number of moles of gas and R is the ideal gas constant.
n=1.10 x 10^5 mol
V= 2.70 x 10^6 L
P= 1.00 atm= 101.325 kPa
R= 8.314 kPa*L/ mol*K
when the formula is rearranged, T=PV/ nR
T = (101.325kPa * 2.70 x 10^6 L)/ (1.10 x 10^5 mol * 8.314 kPa*L/ mol*K)
T = 299.1421917 K
or
T = 299.14 - 273.15 = 25.99 = 26°C
Answer:
C
Explanation:
because it is product over reactants. hope this helps :)
Complete question:
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×10⁻⁴ s⁻¹ at a certain temperature.
If the initial concentration of SO2Cl2 is 0.125 M , what is the concentration of SO2Cl2 after 210 s ?
Answer:
After 210 s the concentration of SO2Cl2 will be 0.121 M
Explanation:
![ln\frac{[A_t]}{[A_0]} =-kt](https://tex.z-dn.net/?f=ln%5Cfrac%7B%5BA_t%5D%7D%7B%5BA_0%5D%7D%20%3D-kt)
where;
At is the concentration of A at a time t
A₀ is the initial concentration of A
k is rate constant = 1.44×10⁻⁴ s⁻¹
t is time
ln(At/A₀) = -( 1.44×10⁻⁴)t
ln(At/0.125) = -( 1.44×10⁻⁴)210
ln(At/0.125) = -0.03024
At/0.125 = 0.9702
At = 0.125*0.9702
At = 0.121 M
Therefore, after 210 s the concentration of SO2Cl2 will be 0.121 M
