Answer: When a substance is pure, it is composed of one type of molecule. For example, table salt is only composed of (more or less) salt molecules, while seawater has water and salt molecules. A more complicated example of a non - pure substance is soil. It has many different types of nutrients and compounds.
Since the half-reaction is occurring in a basic solution, add 32OH− to each side of the equation to eliminate the H+ ions.
P₄ +16H₂O + 32OH⁻ ⟶ 4PO₃⁻⁴ + 32H⁺ +32OH⁻
Final reaction :
P₄ + 32OH⁻ ⟶ 4PO₃⁻⁴ + 16H₂O + 20e⁻
A half reaction is either the oxidation or reduction reaction component of a redox reaction. A half reaction is obtained by considering the change in oxidation states of individual substances involved in the redox reaction.
The concept of half-reactions is used to describe what occurs in an electrochemical cell, such as a Galvanic cell battery. Half-reactions can be written to describe both the metal undergoing oxidation (known as the anode) and the metal undergoing reduction (known as the cathode).
Half-reactions are often used as a method of balancing redox reactions. For oxidation-reduction reactions in acidic conditions, after balancing the atoms and oxidation numbers, one will need to add H+ ions to balance the hydrogen ions in the half reaction.
For oxidation-reduction reactions in basic conditions, after balancing the atoms and oxidation numbers, first treat it as an acidic solution and then add OH- ions to balance the H+ ions in the half reactions (which would give H2O).
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Answer:
Cr (HSO4)3
Explanation:
its molecular weight is 343.20 g/mol
its molecular formula can also be written as CrH3O12S3
molar mass of Cr (HSO4)3 can be calculated by following method;
atomic mass of Cr = 51.9961 u
atomic mass of H = 1 u
atomic mass of S = 32.065 u
atomic mass of O = 16 u
molar mass of Cr(HSO4)3 = 51.9961+ 1.00784×3 + 32.065×3 + 15.999×12
molar mass of Cr(HSO4)3 =51.9961+3.02352+96.195+ 191.988
molar mass of Cr(HSO4)3 = 343.20 g/mol
Answer:
Overall reaction
H2(g) + 2ICI(g) -----> I2(g) +2HCl(g)
Overall Rate = k1[H2] [ICl]
Explanation:
Overall reaction
H2(g) + 2ICI(g) -----> I2(g) +2HCl(g)
The overall reaction is the sum of the two two reactions shown in the question. After the two reactions are summed up properly, this overall reaction equation his obtained.
Since K1<<K2 it means that step 1 is slower than step 2. Recall that the rate if reaction depends on the slowest step of the reaction. Hence
Overall Rate = k1[H2] [ICl]
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
