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Allushta [10]
3 years ago
11

Which of the following is not a catalyst? A. Nickel B. Platinum C. Enzymes D. Phosphorus

Chemistry
2 answers:
Bogdan [553]3 years ago
7 0

Answer:

The correct answer is D. Phosphorus is not a catalyst.

Explanation:

A catalyst is a substance that accelerates a chemical reaction at a certain temperature, but does not itself wear off the reaction. It is involved in the chemical reaction but is not the starting or end product of the reaction.

Catalysts create an alternative reaction pathway for the reaction with a lower activation energy. Activation energy is the energy required for the reaction to take place. However, the catalyst cannot cause a reaction which does not take place without the catalyst.

Depending on the phases in which the catalyst and reactants are present, one speaks of homogeneous or heterogeneous catalysts. Biochemical processes are catalyzed by enzymes, while heterogeneous catalysts are metals, such as platinum and nickel.

Mazyrski [523]3 years ago
6 0
The answer would be D because from my research it's the only one that didn't have a catalyst 
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What mass of gallium oxide, Ga₂O3, can be prepared from
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How did Ernest Rutherford's experiment relate to J.J. Thomson's work?
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3 years ago
If 316 mL nitrogen is combined with 178 mL oxygen, what volume of N2O is produced at constant temperature and pressure if the re
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=259 ml

Explanation;

-According to Gay Lussac's Law of Combining Volumes when gases react, they do so in volumes which have a simple ratio to one another, and to the volume of the product formed if gaseous, provided the temperature and pressure remain constant.

-Thus; from the volume of nitrogen and oxygen gases; we have; 316 / 178 = 1.775 moles of nitrogen gas per mole of oxygen gas.

-Therefore, nitrogen gas is the limiting reactant, and for each mole of nitrogen gas used, we will get 1 mole of N2O. This means the resulting volume of N2O with 100% yield will be the same as the volume of nitrogen gas used, thus, 100% yield will produce 316 mL.

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7 0
3 years ago
Read 2 more answers
5.11 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the
cupoosta [38]

Answer: Thus ∆H, in kJ/mol, for the dissolution of MgSO₄ is -66.7 kJ

Explanation:

To calculate the entalpy, we use the equation:

q=mc\Delta T

where,

q = heat absorbed by water = ?

m = mass of water = {\text {volume of water}}\times {\text {density of water}}=100.0ml\times 1.00g/ml=100.0g

c = heat capacity of water = 4.186 J/g°C

\Delta T= change in temperature = 6.70^0C

q=100.0g\times 4.184J/g^0C\times 6.70^0C=2803.3J=2.8033kJ

Sign convention of heat:

When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.

The heat absorbed by water will be equal to heat released by MgSO_4

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Given mass = 5.11 g

Molar mass  = 120 g/mol

Putting values in above equation, we get:

\text{Moles of }MgSO_4=\frac{5.11g}{120g/mol}=0.042mol

0.042 moles of MgSO_4 releases = 2.8033 kJ

1 mole of MgSO_4 releases = \frac{2.8033 kJ}{0.042}\times 1=66.7kJ

Thus ∆H, in kJ/mol, for the dissolution of MgSO₄ is -66.7 kJ

3 0
3 years ago
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