All categories

2 years ago

Please help

Chemistry

1 answer:

Mazyrski [523]2 years ago

4 0

Answer:

Diagram Z

Explanation:

A cell placed into a hypotonic solution will swell and expand until it eventually burst through a process known as cytolysis.

You might be interested in

carbon disulfide is formed by the reaction of coke (carbon) with sulfur dioxide. how many moles of cs2 will be generated if 8.0

Murrr4er [49]

5C₂ + 4SO₂ ------> 2CS₂ + 8CO

mole ratio of C₂ : CS₂
=   5 : 2

∴ since C₂ contains 8 moles

then CS₂ contain    $( \frac{8}{5} ) * 2$ moles

= 3.2 moles

7 0

2 years ago

What mass of CO is needed to react completely with55.0 g of Fe2O3(s)+CO(g) yield Fe(s)+CO2(g)?

Katarina [22]

Answer:

28.9 g

Explanation:

We know that we will need a balanced equation with masses, moles, and molar masses of the compounds involved.

<em>Gather all the information in one place</em> with molar masses above the formulas and masses below them.

$M_{r}$ : 159.69 28.01

Fe₂O₃ + 3CO ⟶ 2Fe + 3CO₂

Mass/g: 55.0

1. Use the molar mass of Fe₂O₃ to calculate the moles of Fe₂O₃.

$\text{Moles of Fe$_{2}$O$_{3}$} =\text{55.0 g Fe$_{2}$O$_{3}$} \times \frac{\text{1 mol Fe$_{2}$O$_{3}$}}{\text{159.69 g Fe$_{2}$O$_{3}$}}= \text{0.3444 mol Fe$_{2}$O$_{3}$}$

2. Use the molar ratio of CO:Fe₂O₃ to calculate the moles of CO.

$\text{Moles of CO} = \text{0.3444 mol Fe$_{2}$O$_{3}$} \times \frac{\text{3 mol CO}}{\text{1 mol Fe$_{2}$O$_{3}$}}= \text{1.033 mol CO}$

3.Use the molar mass of CO to calculate the mass of CO.

$\text{Mass of CO} = \text{1.033 mol CO} \times \frac{\text{28.01 g CO} }{\text{1 mol CO}}= \textbf{28.9 g CO}$

3 0

2 years ago

Read 2 more answers

How do scientists test ideas about chemical evolution?

maksim [4K]

I think they test ideas about chemical evolution by doing experiments. Hope this helps

4 0

3 years ago

Read 2 more answers

1) The heat of combustion for the gases hydrogen, methane and ethane are −285.8, −890.4 and −1559.9 kJ/mol respectively at 298K.

Morgarella [4.7K]

Answer:

The enthalpy of the reaction is 64.9 kJ/mol.

Explanation:

$H_2 + \frac{1}{2}O_2\rightarrow H_2O,\Delta H_1 =-285.8 kJ$ ..[1]

$CH_4 + 2O_2\rightarrow CO_2 + 2H_2O,\Delta H_2 =-890.4 kJ$ ..[2]

$C_2H_6 + \frac{7}{2}O_2\rightarrow 2CO_2 + 3H_2O,\Delta H_3= -1559.9 kJ$ ..[3]

$2CH_4(g)\rightarrow C_2H_6(g) + H_2(g),\Delta H_4=?$ ..[4]

2 × [2] - [1]- [3] = [4] (Using Hess's law)

$\Delta H_4=2\times \Delta H_2 -\Delta H_1 -\Delta H_3$

$\Delta H_4=2\times (-890.4 kJ)-(-285.8 kJ) -(-1559.9 kJ)$

$\Delta H_4=64.9 kJ/mol$

The enthalpy of the reaction is 64.9 kJ/mol.

3 0

2 years ago

can someone help me more clearly understand the difference between heterogeneous and homogeneous? Give an example of each plz.

const2013 [10]

Heterogenous mixtures are unevenly mixed. Like oil and vinegar in vinaigrette if it is not emulsified well enough and they separate. Any case where two things are not evenly distributed within each other.

Homogenous mixtures are evenly mixed throughout. Like salt water or kool-aid (when it's mixed).

Hope this helps!

3 0

3 years ago