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klemol [59]
3 years ago
10

Which statement indicates that a substance may be an ionic compound?

Chemistry
1 answer:
Free_Kalibri [48]3 years ago
4 0
It can be flattened with force and is made up of crystal lattice.
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What is the difference between measured and accepted value? And how are these values used to determine the precision of these va
serg [7]
Measured values are verified and go under a series of experiments before being accepted as the norm. Accepted values are unanimously accepted values, seen as the norm by a qualified group of individuals (scientists or the people of the intellectual sphere).
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3 years ago
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An increasing population will create an increasing demand for fossil fuels. The burning of fossil fuels can
Inessa [10]

Answer:

//

Explanation:

it's C = Sulphur Dioxide

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Urea is a common fertilizer with the formula CO(NH2)2 that is sometimes used as a chemical de-icer for icy road surfaces in the
nordsb [41]

Answer:

The answer to your question is  molality = 0.61

Explanation:

Freezing point is the temperature at which a liquid turns into a solid if a solute is added to a solution, the freezing point changes.

Data

Kf = 1.86 °C/m

molality = ?

ΔTc = 1.13°C

Formula

ΔTc = kcm

Solve for m

m = ΔTc/kc

Substitution

m = 1.13 / 1.86

Simplification and result

m = 0.61

4 0
4 years ago
Assuming that the bath contains 250.0 g of water and that the calorimeter itself absorbs a negligible amount of heat, calculate
Anvisha [2.4K]

Answer:

-3272     kJ/mol

Explanation:

Given and known facts

Mass of Benzene = 0.187 grams

Mass of water = 250 grams

Standard heat capacity of water = 4.18 J/g∙°C

Change in temperature ΔT = 7.48°C

Heat

=250 * 4.18 * 7.48\\=7816.6 \\=7.82

Heat released by benzine is - 7.82 kJ

Now, we know that

0.187 grams of benzene release = -7.82  kJ heat

So, 1 g benzine releases

\frac{ -7.82 }{0.187}\\= -41.8

kJ/g

0.187 * \frac{1}{78.108}=0.00239 mol C6H6

Heat released

= \frac{-7.82}{ 0.00239}

=-3272     kJ/mol

4 0
3 years ago
What pressure (in atm) will a sample of o2 gas occupy at 100.0 ml, if o2 has a volume of 25.00 ml at 2.0 atm?
xeze [42]

Assuming that the O2 gas acts like an ideal gas, we find the following expression to be approximates of the behaviour of this gas:

<span>P V = n R T                   ---> 1</span>

where,

P = pressure exerted by the gas

V = volume occupied

n = number of moles

R = universal gas constant

T = absolute temperature

Further, we assume that the number of moles and the temperature are constant, hence reducing equation 1 into the form:

<span>P V = k                         ---> 2</span>

where k is a constant. Therefore we can equate two states:

P1 V1 = P2 V2

Since P1, V1 and V2 are given and we are to look for P2:

25 mL * 2 atm = 100 mL * P2

<span>P2 = 0.5 atm</span>

8 0
3 years ago
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