How many oxygen atoms are present in 8.186*10-20 g of hclo4?

-. Convert 54 m to its equivalent measurement in cm.

Sergio [31]

Answer:

5400 cm

Explanation:

$\huge \because \: 1 \: m = 100 \: cm \\ \\ \huge \therefore \: 54 \: m = 54 \times 100 \\ \\ \: \huge \therefore \: 54 \: m= 5400 \: cm$

6 0

3 years ago

If all data points lie in a straight line on your standard curve except for one point. Should you ignore the point or shift the

Ivanshal [37]

Ignore the point, the majority of the points are along the trend line.

3 0

3 years ago

Read 2 more answers

Does anybody know how to do q4. Please show working out thanks.

insens350 [35]

Answer:

% purity of limestone = 96.53%

Explanation:

Question (4).

Weight of impure CaCO₃ = 25.9 g

Molecular weight of CaCO₃ = 40 + 12 + 3(16)

= 100 g per mole

We know at S.T.P. number of moles of CO₂ = 1 and volume = 22.4 liters

From the given reaction, 1 mole of CaCO₃ reacts with 1 mole or 22.4 liters of

CO₂.

∵ 22.4 liters of CO₂ was produced from CaCO3 = 100 g

∴ 1 liter of CO₂ will be produced by CaCO₃ = $\frac{100}{22.4}$

∴ 5.6 liters of CO₂ will be produced by CaCO₃ = $\frac{100\times 5.6}{22.4}$

= 25 g

Therefore, % purity of CaCO₃ = $\frac{\text{Weight calculated}}{{\text{Weight given}}}\times 100$

= $\frac{25}{25.9}\times 100$

= 96.53 %

7 0

3 years ago

What is the chemical name for Se8O7

irina1246 [14]

Answer:

Selenium oxide

Explanation:

3 0

2 years ago

6. How many moles of water would require 92.048 kJ of heat to raise its temperature from 34.0 °C to 100.0 °C? (3 marks)

scoray [572]

Taking into account the definition of calorimetry, 0.0185 moles of water are required.

<h3>Calorimetry</h3>

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

Sensible heat is defined as the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).

So, the equation that allows to calculate heat exchanges is:

Q = c× m× ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

<h3>Mass of water required</h3>

In this case, you know:

Heat= 92.048 kJ
Mass of water = ?
Initial temperature of water= 34 ºC
Final temperature of water= 100 ºC
Specific heat of water = 4.186 $\frac{J}{gC}$

Replacing in the expression to calculate heat exchanges:

92.048 kJ = 4.186 $\frac{J}{gC}$ × m× (100 °C -34 °C)

92.048 kJ = 4.186 $\frac{J}{gC}$ × m× 66 °C

m= 92.048 kJ ÷ (4.186 $\frac{J}{gC}$ × 66 °C)

<u><em>m= 0.333 grams</em></u>

<h3>Moles of water required</h3>

Being the molar mass of water 18 $\frac{g}{mole}$ , that is, the amount of mass that a substance contains in one mole, the moles of water required can be calculated as:

$amount of moles=0.333 gramsx\frac{1 mole}{18 grams}$

<u><em>amount of moles= 0.0185 moles</em></u>

Finally, 0.0185 moles of water are required.

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8 0

2 years ago