High temperature and pressure produce the highest rate of reaction. However, this must be balanced with the high cost of the energy needed to maintain these conditions. Catalysts increase the rate of reaction without affecting the yield. This can help create processes which work well even at lower temperatures.
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Uranium-235 would be more useful for dating in Cambrian time because Cambrian time was 540 million years ago while the half life of carbon-14 is only 5,730 years
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For balancing acidic solutions, we would need to add H+ ions to the correct side of the equation to balance the total number of atoms and the overall charge.
Answer:
C.) At room temperature and pressure, because intermolecular interactions are minimized and the particles are relatively far apart.
Explanation:
For gas to behave as an ideal gas there are 2 basic assumptions:
- The intermolecular forces (IMF) are neglectable.
- The volume of the gas is neglectable in comparison with the volume of the container.
<em>In which instance is a gas most likely to behave as an ideal gas?</em>
<em>A.) At low temperatures, because the molecules are always far apart.</em> FALSE. At low temperatures, molecules are closer and IMF are more appreciable.
<em>B.) When the molecules are highly polar, because IMF are more likely.</em> FALSE. When IMF are stronger the gas does not behave as an ideal gas.
<em>C.) At room temperature and pressure, because intermolecular interactions are minimized and the particles are relatively far apart.</em> TRUE.
<em>D.) At high pressures, because the distance between molecules is likely to be small in relation to the size of the molecules.</em> FALSE. At high pressures, the distance between molecules is small and IMF are strong.
The answer for the following problem is mentioned below.
- <u><em>Therefore the final moles of the gas is 14.2 × </em></u>
<u><em> moles.</em></u>
Explanation:
Given:
Initial volume (
) = 230 ml
Final volume (
) = 860 ml
Initial moles (
) = 3.8 × moles
To find:
Final moles (
)
We know;
According to the ideal gas equation;
P × V = n × R × T
where;
P represents the pressure of the gas
V represents the volume of the gas
n represents the no of the moles of the gas
R represents the universal gas constant
T represents the temperature of the gas
So;
V ∝ n
= 
where,
() represents the initial volume of the gas
() represents the final volume of the gas
() represents the initial moles of the gas
() represents the final moles of the gas
Substituting the above values;
= 
= 14.2 × moles
<u><em>Therefore the final moles of the gas is 14.2 × </em></u><u><em> moles.</em></u>
