Physical changes are changes affecting the form of a chemical substance, but not it's chemical composition.
31,000 milligrams is equal to 31 grams
I think it is D but im not sure
Answer:
69% Ag, 10.5% S, 20.5% O.
Explanation:
Ag₂SO₄ → Molar mass = 311.8 g/mol
2 mol of Ag → 107.87g/m . 2m = 215.74 g
1 mol of S → 32.06g/m . 1m = 32.06 g
4 mol of O → 16g/m .4m = 64 g
Percentage composition will be:
(Mass of Ag/ Total mass) . 100
(215.74 g / 311.8 g) . 100 = 69 %
(Mass of S/ Total mass) . 100
(32.06 g / 311.8 g) .100 = 10.5%
(Mass of O/ Total mass) . 100
(64 g / 311.8 g) . 100 = 20.5 %
Answer:
Option D. atm, L, K, mole
Explanation:
To know which option is correct, do the following:
We shall use the standard value for each variable to obtain the gas constant. This can be obtained as follow:
Volume (V) = 22400 mL
Pressure (P) = 760 mmHg
Number of mole (n) = 1 mole
Temperature (T) = 273 K
Gas constant (R) =?
PV = nRT
R = PV / nT
R = (760 × 22400) / (1 × 273)
R = 62358.97 mmHg.mL/Kmol
Volume (V) = 22.4 L
Pressure (P) = 760 mmHg
Number of mole (n) = 1 mole
Temperature (T) = 273 K
Gas constant (R) =?
PV = nRT
R = PV / nT
R = (760 × 22.4) / (1 × 273)
R = 62.359 mmHg.L/Kmol
Volume (V) = 22400 mL
Pressure (P) = 1 atm
Number of mole (n) = 1 mole
Temperature (T) = 273 K
Gas constant (R) =?
PV = nRT
R = PV / nT
R = (1 × 22400) / (1 × 273)
R = 82.05 atm.mL/Kmol
Volume (V) = 22.4 L
Pressure (P) = 1 atm
Number of mole (n) = 1 mole
Temperature (T) = 273 K
Gas constant (R) =?
PV = nRT
R = PV / nT
R = (1 × 22.4) / (1 × 273)
R = 0.0821 atm.L/Kmol
From the above illustrations, we can see that the gas constant will have a value for 0.0821 as long as other variables are: atm, L, K, mole
