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3 years ago

What do animal and plant cells have in common

Chemistry

1 answer:

Pavlova-9 [17]3 years ago

6 0

Answer:

both have cell membranes

Explanation:

the animal cell has small or temporary vacuoles.

animal cell does not have chloroplast or cell wall.

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. What is the mass of 23.56 moles of Glucose ples of Glucose - C6H1206?

GaryK [48]

Answer:

4244.48 g to the nearest hundredth.

Explanation:

The molar mass of Glucose = 6*12.011 + 12*1.008+ 6*15.999

= 180.156.

So 23.56 moles = 180.156 * 23.56 = 4244.48 g

8 0

4 years ago

How is the pH of an acidic substance raised?

BabaBlast [244]

Answer: 4) Concentrate it

Explanation:

4 0

3 years ago

What volume of sample, in mL, would be needed to make 2 mL of a 5-fold dilution? (3 significant figures needed)

natulia [17]

Answer:

0.400 mL

Explanation:

Hello, the dilution factor (in folds) is given by:

$folds=\frac{total_{volume}}{sample_{volume}}$

Thus, the sample volume with three significant figures is given by:

$sample_{volume}=\frac{2mL}{5"folds"}=0.400 mL$

Best regards.

5 0

3 years ago

Which of the following has kinetic energy? Wind blowing at 3 km/h A fully stretched elastic band A boulder sitting on top of a h

ser-zykov [4K]

Answer: i might be wrong but i feel like it’s A. wind blowing at 3km/h just because “ energy of an object is the energy that it possesses due to its motion.”

Explanation:

4 0

3 years ago

Read 2 more answers

Consider a galvanic cell based on the reaction Al^3+_(aq) + Mg_(s) rightarrow Al_(s) + Mg^2+ _(aq) The half-reactions are Al^3+

grin007 [14]

Answer: The standard cell potential of the cell is -0.71 V

Explanation:

The half reactions follows:

Oxidation half reaction: $Mg\rightarrow Mg^{2+}+2e^-;E^o_{Mg^{2+}/Mg}=-2.37V$ ( × 3)

Reduction half reaction: $Al^{3+}(aq.)+3e^-\rightarrow Al(s);E^o_{Al^{3+}/Al}=-1.66V$ ( × 2)

The balanced cell reaction follows:

$2Al^{3+}(aq.)+3Mg(s)\rightarrow 2Al(s)+3Mg^{2+}(aq.)$

To calculate the $E^o_{cell}$ of the reaction, we use the equation:

$E^o_{cell}=E^o_{cathode}-E^o_{anode}$

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

Putting values in above equation, we get:

$E^o_{cell}=-2.37-(-1.66)=-0.71V$

Hence, the standard cell potential of the cell is -0.71 V

8 0

3 years ago