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GarryVolchara [31]
3 years ago
9

M=40g V=31cm^3 what is the density

Chemistry
1 answer:
zepelin [54]3 years ago
4 0
40g/31cm^3=1.3g/cm^3
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third point

Explanation:

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What does ClF3 stand for
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If I mix bleach and namona and throw it on a person what will happen​
satela [25.4K]

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They have the chance to inhale toxic fumes secreted by the mixture.

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7 0
3 years ago
You have collected a tissue specimen that you would like to preserve by freeze drying. To ensure the integrity of the specimen,
Reika [66]

Answer:

The maximum pressure is 612.2 Pa

Explanation:

The pressure of the ice (P1) = 624 Pa

The temperature of the ice = 273.16 K

The maximum temperature the specimen = - 5 oC

                                                                     = -5 + 273 = 268K

The maximum Pressure the freeze drying can be will be (P2) = ?

Using Pressure law, which shows the relationship between pressure and temperature.

                        P1 / T1 = P2 / T2

                       P2 T1 = P1 T2

                       P2 = P1 T2 / T1

                       P2 = 624 × 268 / 273.16

                       P2 = 612.2 Pa

The maximum pressure at which drying can be carried out is 612.2 Pa

Check the attached document more explanation.   jjjjggggg

5 0
3 years ago
The equilibrium 2NO(g)+Cl2(g)⇌2NOCl(g) is established at 500 K. An equilibrium mixture of the three gases has partial pressures
QveST [7]

<u>Answer:</u>

<u>For A:</u> The K_p for the given reaction is 4.0\times 10^1

<u>For B:</u> The K_c for the given reaction is 1642.

<u>Explanation:</u>

The given chemical reaction follows:

2NO(g)+Cl_2(g)\rightleftharpoons 2NOCl(g)

  • <u>For A:</u>

The expression of K_p for the above reaction follows:

K_p=\frac{(p_{NOCl})^2}{(p_{NO})^2\times p_{Cl_2}}

We are given:

p_{NOCl}=0.24 atm\\p_{NO}=9.10\times 10^{-2}atm=0.0910atm\\p_{Cl_2}=0.174atm

Putting values in above equation, we get:

K_p=\frac{(0.24)^2}{(0.0910)^2\times 0.174}\\\\K_p=4.0\times 10^1

Hence, the K_p for the given reaction is 4.0\times 10^1

  • <u>For B:</u>

Relation of K_p with K_c is given by the formula:

K_p=K_c(RT)^{\Delta ng}

where,

K_p = equilibrium constant in terms of partial pressure = 4.0\times 10^1

K_c = equilibrium constant in terms of concentration = ?

R = Gas constant = 0.0821\text{ L atm }mol^{-1}K^{-1}

T = temperature = 500 K

\Delta ng = change in number of moles of gas particles = n_{products}-n_{reactants}=2-3=-1

Putting values in above equation, we get:

4.0\times 10^1=K_c\times (0.0821\times 500)^{-1}\\\\K_c=\frac{4.0\times 10^1}{(0.0821\times 500)^{-1})}=1642

Hence, the K_c for the given reaction is 1642.

7 0
3 years ago
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