All categories

3 years ago

What part of the plant is fertilized with pollen to produce seeds?

Chemistry

2 answers:

Radda [10]3 years ago

6 0

Ovule is the answer

ella [17]3 years ago

5 0

Answer:

Ovule

Explanation:

You might be interested in

Removing one electron from an atom results in the formation of an

STatiana [176]

Ion with a 1+ charge. The atom would normally be neutral, since it has the same number of electrons as it does protons; removing an electron leaves one more proton than electron. Since protons are positive and there's one more of them than electrons in the new ion, it has a 1+ charge.

5 0

3 years ago

Read 2 more answers

Which of the following is an example of a way you can reduce personal consumption of resources?

dsp73

Answer:

B. using efficient light bulbs

4 0

3 years ago

Ferns and reptiles appeared in the____ era

Kay [80]

Ferns and reptiles appeared in the paleozoic era.

5 0

4 years ago

Read 2 more answers

PLEASE HELP! 25 POINTS!!!! I got the #1, just not #2 and #3. An industrial chemical company has opened a new plant that will pro

podryga [215]

Answer :

Part 1 : Balanced reaction, $3H_2(g)+N_2(g)\rightarrow 2NH_3(g)$

Part 2 : The theoretical yield of $NH_3$ gas = 440.96 g

Part 3 : The % yield of ammonia is 90.03 %

Solution : Given,

Mass of $N_2$ = 475 g

Molar mass of $N_2$ = 28 g/mole

Molar mass of $NH_3$ = 17 g/mole

Experimental yield of $NH_3$ = 397 g

Answer for Part (1) :

The balanced chemical reaction is,

$3H_2(g)+N_2(g)\rightarrow 2NH_3(g)$

Answer for Part (2) :

First we have to calculate the moles of $N_2$ .

$\text{Moles of }N_2=\frac{\text{ Mass of }N_2}{\text{ Molecular mass of }N_2}=\frac{475g}{28g/mole}=16.96moles$

From the given reaction, we conclude that

1 moles of $N_2$ gas react to give 2 moles of $NH_3$ gas

16.96 moles of $N_2$ gas react to give $\frac{2}{1}\times 16.96=33.92$ moles of $NH_3$ gas

Now we have to calculate the mass of $NH_3$ gas.

$\text{ Mass of }NH_3=\text{ Moles of }NH_3\times \text{ Molar mass of }NH_3$

$\text{ Mass of }NH_3=(33.92moles)\times (17g/mole)=440.96g$

Therefore, the theoretical yield of $NH_3$ gas = 440.96 g

Answer for Part (3) :

Formula used for percent yield :

$\% \text{ yield of }NH_3=\frac{\text{ Experimental yield of }NH_3}{\text{ Theoretical yield of }NH_3}\times 100$

$\% \text{ yield of }NH_3=\frac{397g}{440.96g}\times 100=90.03\%$

Therefore, the % yield of ammonia is 90.03 %

3 0

3 years ago

An aqueous solution is 0.387 m in hcl. what is the molality of the solution if the density is 1.23 g/ml?

vazorg [7]

Assume you have 1.00 L (1000 mL) of solution. d = m / V m = d x V = 1.23 g/mL x 1000 mL = 1230 g of solution 0.387 mol/L x 1 L = 0.387 mol HCl 0.387 mol HCl x (36.5 g / 1 mol) = 14.1 g HCl mass of water = 1230 g solution - 14.1 g HCl = 1216 g H2O = 1.216 kg H2O molality = mol HCl / kg water = 0.387 mol / 1.216 kg = 0.318 mol/kg (or 0.318 molal)

8 0

3 years ago