Main Answer:
Given data:
Mass of ice m = 12 grams = 12/1000 = 0.012 kg
Specific heat s = 4.18 KJ/ gm-1 C-1
Change in temperature t = t2 - t1
t = 100 - (-10)
t = 100 + 10 = 110C
Heat required Q = m x s x t
Q = 0.012 x 4.18 x 110
Q = 5.5176 KJ
Explanation:
What is heat?
Heat is defined as one of the forms of energy. It is a kinetic energy which can be transferred from one object to another object or medium. It cannot be destroyed or created. The units of heat is Joules in SI system and calories in CGS system.
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When an atom or molecule accepts or looses an electron or electrons it gets either negative charge (when electrons gained) or a positive charge (when looses electron). The negative ion is called Anion and positve ion is called the Cation. An Ion can be Atomic or Polyatomic.
Example:
Sodium when looses one electron forms a cation i.e. Na⁺
Chlorine when gains one electron forms an Anion i.e. Cl⁻
Result:
<span>A negative ion (Anion) differ from an uncharged atom of the same element in the number of electrons. An anion contains more electrons than its corresponding Neutral Element.</span>
Answer:
70%of 2000 = 1400
2000 tonnes of hematite contains 1400 tonnes iron oxide .
1400 tonnes of fe2O3
fe2O3 have molar mass 159.69
calculate moles = given mass/molar mass
moles = 1400000000/159.69
moles = 8766986
one mole contains = 112 g of fe
so 8766986 moles will contain = 112×8766986
= 981,902,432 grams of ferrous
which is nothing but equal to 981.90 tonnes of iron!!
Ka x Kb = Kw Kw = 1 x 10⁻¹⁴
(1.3 x 10⁻⁷) x Kb = 1 x 10⁻¹⁴
Kb = ( 1 x 10⁻¹⁴ ) / ( 1.3 x 10⁻⁷)
Kb = 7.7 x 10⁻⁸
Answer D
hope this helps!
You need to use the % information to determine the empirical formula of the compound first.
The empirical formula is the simplest ratio of atoms in the molecule.
Then use the rest of the data to determine moles of gas, and use this to determine molar mass of gas...
Empirical formula calculations:
Assume you have 100 g, calculate the moles of each atom in the 100 g
moles = mass / molar mass
molar mass C = 12.01 g/mol
molar mass H = 1.008 g/mol
molar mass O = 16.00 g/mol
C = 64.9 % = 64.6 g
H = 13.5 % = 13.5 g
O = 21.6 % = 21.6 g
moles C = 64.6 g / 12.01 g/mol = 5.38 mol
moles H = 13.5 g / 1.008 g/mol = 13.39 mol
moles O = 21.6 g / 16.00 g/mol = 1.35 mol
So ratio of C : H : O
is 5.38 mol : 13.39 mol : 1.35 mol
Divide each number in the ratio by the lowest number to get the simplest whole number ratio
(5.38 / 1.35) : (13.39 / 1.35) : (1.35 / 1.35)
4 : 10 : 1
empirical formula is
C4H10O
Finding moles and molar mass calcs
Now, you know that at 120 deg C and 750 mmHg that 1.00L compound weighs 2.30 g.
We can use this information to determine the molar mass of the gas after first working out how many moles the are in the 1.00 L
PV = nRT
P = pressure = 750 mmHg
V = volume = 1.00 L
n = moles (unknown)
T = temp in Kelvin (120 deg C = (273.15 + 120) Kelvin)
- T = 393.15 Kelvin
R = gas constant, which is 62.363 mmHg L K^-1 mol^-1 (when your P is in mmHg and volume is in L)
n = PV / RT
n = (750 mmHg x 1.00 L) / (62.363mmHg L K^-1 mol^-1 x 393.15 K)
n = 0.03059 moles of gas
We know moles = 0.03509 and mass = 2.30 g
So we can work out molar mass of the gas
moles = mass / molar mass
Therefore molar mass = mass / moles
molar mass = 2.30 g / 0.03059 mol
= 75.19 g/mol
Determine molecular formula
So empirical formula is C4H10O
molar mass = 75.19 g/mol
To find the molecular formula you divide the molar mass by the formula weight of the empirical formula...
This tells you how many times the empirical formula fits into the molecular formula. Tou then multiply every atom in the empirical formula by this number
formula weight C4H10O = 74.12 g/mol
Divide molar mass by formula weight empirical
75.15 g/mol / 74.12 g/mol
= 1
(It doesn't matter that the number don't quite match, they rarely do in this type of calc (although I could have made a slight error somewhere) but the numbers are very close, so we can say 1.)
The empirical formula only fits into the molar mass once,
molecular formula thus = empirical formula
<span>
C4H10O
Therefore, the </span>molecular formula of the compound is <span>C4H10O.
I hope my answer has come to your help. Thank you for posting your question here in Brainly. We hope to answer more of your questions and inquiries soon. Have a nice day ahead!</span>
