Answer:
Rate of reaction = -d[D] / 2dt = -d[E]/ 3dt = -d[F]/dt = d[G]/2dt = d[H]/dt
The concentration of H is increasing, half as fast as D decreases: 0.05 mol L–1.s–1
E decreseas 3/2 as fast as G increases = 0.30 M/s
Explanation:
Rate of reaction = -d[D] / 2dt = -d[E]/ 3dt = -d[F]/dt = d[G]/2dt = d[H]/dt
When the concentration of D is decreasing by 0.10 M/s, how fast is the concentration of H increasing:
Given data = d[D]/dt = 0.10 M/s
-d[D] / 2dt = d[H]/dt
d[H]/dt = 0.05 M/s
The concentration of H is increasing, half as fast as D decreases: 0.05 mol L–1.s–1
When the concentration of G is increasing by 0.20 M/s, how fast is the concentration of E decreasing:
d[G] / 2dt = -d[H]/3dt
E decreseas 3/2 as fast as G increases = 0.30 M/s
a specific hypothesis to test with a controlled experiment
population is the number of species living in a given area if this is regarding biology or earth studies :)
During photosynthesis, 5 moles of water are needed to produce 150 grams of glucose. The correct option is D.
<h3>What is photosynthesis?</h3>
It is the process by which green plants and some other organisms use sunlight to synthesize nutrients from carbon dioxide and water.
- Step 1: Write the balanced equation for photosynthesis.
6 CO₂ + 6 H₂O ⇒ C₆H₁₂O₆ + 6 O₂
- Step 2: Convert 150 g of C₆H₁₂O₆ to moles.
The molar mass of C₆H₁₂O₆ is 180.16 g/mol.
150 g × 1 mol/180.16 g = 0.833 mol
- Step 3: Calculate the moles of water required to form 0.833 moles of C₆H₁₂O₆
The molar ratio of H₂O to C₆H₁₂O₆ is 6:1.
0.833 mol C₆H₁₂O₆ × 6 mol H₂O/1 mol C₆H₁₂O₆ = 5.00 mol H₂O
During photosynthesis, 5 moles of water are needed to produce 150 grams of glucose. The correct option is D.
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As a result, the greatest number of an atom's oxidation state will gradually rise over each period of the periodic table. For instance, the third period's highest value of the oxidation number will fall between 1 and 7.
- The Periodic Table only consistently varies the oxidation numbers of Group 1 and Group 2 metals in their compounds, which are always +1 and +2, respectively.
- Elements have an increasing number of valence electrons that can range from 1 to 8 and move from left to right over time. However, when H or O are added to an element first, the element's valency rises to 4, then falls to zero.
<h3>What causes a rise in the oxidation number?</h3>
An increase in oxidation number results from the loss of negatively charged electrons, whereas a reduction in oxidation number results from the gain of electrons. The result is a rise in the oxidation number of the oxidized element or ion.
<h3>Pattern of the Period 2?</h3>
The trends in Period 2 are significantly more clear-cut. All elements in period 2 experience a decrease in atomic radius, an increase in electronegativity, and an increase in ionization energy as their atomic number rises.
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