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aleksklad [387]

2 years ago

9

The descriptions below explain two ways that water is used by plants on a sunny day.

1 answer:

lubasha [3.4K]2 years ago

3 0

In a sunny day, the plant makes use of water through photosynthesis and transpiration.

<h3>What is photosynthesis?</h3>

Photosynthesis is defined as the process by which green plants, which has chlorophyll, makes use of water and carbondioxide in the presence of sunlight as energy to form oxygen and glucose.

Transpiration is the movement is of water out of the plant through its pores located on the leaves, roots and stem. This process is increased in sunny seasons.

Therefore, In a sunny day, the plant makes use of water through photosynthesis and transpiration.

Learn more about photosynthesis here:

brainly.com/question/19160081

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How many moles would be in 85.OmL of 0.750M KOH?

Harlamova29_29 [7]

Answer: There are 0.0637 moles present in 85.0 mL of 0.750 M KOH.

Explanation:

Given: Volume = 85.0 mL (1 mL = 0.001 L) = 0.085 L

Molarity = 0.750 M

It is known that molarity is the number of moles of solute present in liter of a solution.

Therefore, moles present in given solution are calculated as follows.

$Molarity = \frac{moles}{Volume (in L)}\\0.750 M = \frac{moles}{0.085 L}\\moles = 0.0637 mol$

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3 years ago

Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation: N2 1 g 2 1 3H2 1 g

bekas [8.4K]

Answer:

Mass of NH3 produced = 1217 g or 1.217*10^3 g

Explanation:

<u>Given:</u>

Mass of N2 = 1.003*10^3 g

Mass of H2 = 5.003*10^2 g

<u>To determine:</u>

Maximum mass of NH3 that can be produced when the given amounts of N2 and H2 combine

<u>Calculation:</u>

The chemical reaction corresponding to the production of ammonia is:

$N2(g)+3H2(g)\rightarrow 2NH3(g)$

Based on the reaction stoichiometry:

1 mole of N2 combines with 3 moles of H2 to form 2 moles of NH3

$moles\ of\ N2 = \frac{Mass\ N2}{Molar\ mass N2} = \frac{1.003*10^{3}g }{28g/mol} =35.8\ moles$

$moles\ of\ H2 = \frac{Mass\ H2}{Molar\ mass H2} = \frac{5.003*10^{2}g }{2g/mol} =250\ moles$

Since the moles of N2 is less than that of H2, the limiting reagent will be N2 which would in turn determine the amount of NH3 formed.

Based on the reaction stoichiometry the N2 : NH3 ratio = 1:2

Therefore,

$moles\ of\ NH3\ produced = 2*35.8 = 71.6\ moles\\\\Mass\ of\ NH3\ produced = moles*molar mass = 71.6\ moles*17\ g/mol = 1217 g$

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